Welcome To Science Ms. Lara Room A-8 EXAMPLE!! 1 ...t1lara.weebly.com/uploads/1/6/3/2/1632178/0_vhsintromatter_pdf.pdf · Ms. Lara Room A-8. Review Class Syllabus. Learning How To

1. Backpacks/purses in

designated areaThank You!

2. Please take 2 pieces of paper,

a pencil, & syllabus

3. Find the element desk that

matches your element card.

4. Sit in the proper desk.

5. Next, write your name on the

element sheetIll use this for

attendance for today.

EXAMPLE!!

Welcome To Science

Ms. Lara Room A-8

Review Class Syllabus

Learning How To Complete

A Vocabulary Outline

Chemistry

Ch 1 Outline

The following format must be followed in order to receive

full credit:

Write your name and period number at the top right.

Write the title of the vocabulary outline at the top middle

of the page.

Line one will state the number of vocabulary & concepts.

The vocabulary lists will be located at the end of each

chapter. For example, go to page 33 in the textbook (note

next slide)

Name

Period #

Ch 1 Outline (pg 33)

22 Vocabulary + 14 Concepts = 36 Points

Name

Period #



(Page 33)

Note 14

Key Concepts

Note 22

Vocabulary

Name

Period #



Example:

1. analytical chemistry (pg. 8) is the area of study

that focuses on the composition of matter.

1.1 Chemistry

Everything is made of matter & chemistry affects all

aspects of life.

Follow the format below for full credit:

To the left of the vocabulary word/phrase write the

number.

Underline the vocabulary word/phrase, include the

page number.

Summarize the definition. Then repeat the process

for the next vocabulary word/phrase.

Name

Period #



1. analytical chemistry (pg. 8) is the area of study that

focuses on the composition of matter.

Example: pg. 8 in your textbook

1. analytical chemistry (pg. 8) is the area of study

that focuses on the composition of matter.

Summarize the Key Concept bullets (note pg. 33).

Include the subtitles & correct number of bullets.

1.1 Chemistry

Everything is made of matter & chemistry affects

all aspects of life.

Example:

1. analytical chemistry (pg. 8) is the area of

study that focuses on the composition of matter.

1.1 Chemistry

Everything is made of matter & chemistry affects

all aspects of life.

The vocabulary outlines will count as a quiz

grade, no late vocabulary outlines will be

accepted, no exceptions.

Ch 1 Vocabulary Points: 22

Ch 1 Key Concepts Points: 14

= 36 total points

Biology

Ch 1 Outline

The following format must be followed in order to receive

full credit:

Write your name and period number at the top right.

Write the title of the vocabulary outline at the top middle

of the page.

Line one will state the number of vocabulary & concepts.

The vocabulary lists will be located at the end of each

chapter. For example, go to page 30 in the textbook (note

next slide)Name

Period #



Name

Period #



(Page 30)

Note 7 total

Key Concepts

Note 24 total

Vocabulary

Summarize the Key Concept bullets (note pg. 30). Include

the subtitles & correct number of bullets.

Name

Period #



1.1 What Is Science?

The goal of science is to investigate and understand &

explain the natural world and to make useful predictions.

Follow the format below for full credit:

To the left of the vocabulary word/phrase write the

number, underline the vocabulary word/phrase,

(include the page number), Summarize the

definition. Then repeat the process. NamePeriod #



1.1 What Is Science?

The goal of science is to investigate and understand &

explain the natural world and to make useful predictions.

1. science (pg. 3) an organized way of using evidence to

learn about the natural world.


1. science (pg. 3) an organized way of using

evidence to learn about the natural world.




Ch 1 Vocabulary Points: 24

Ch 1 Key Concepts Points: 7

= 31 total points

Chemistry

Ch 2 Outline

(Page 57)

Note: Key

Concepts

Note:

Vocabulary

The following format must be followed in

order to receive full credit:

To the left of the vocabulary word/phrase write

the number.

Next, Underline the vocabulary word/phrase,

include the page number to find the definition.

Find the definition in the textbook & write the

definition next to the vocabulary word/phrase.

Then repeat the process for the next vocabulary

word/phrase.


1. Chemical Change (pg. 48): a change that

produces matter with a different composition.

Once you are finished with the vocabulary list,

summarize the Key Concepts (note pg. 57).




Ch 2 Points: 28 Vocab. + 12 Key Concepts

= 40 total points

Ch 10.3 Points: 1 Vocab. + 3 Key Concepts

= 4 total points

If you get finished with an assignment early

during class, finish the vocabulary outline by

using the online textbook.

Ch 1.1 and 1.2

What Is Chemistry?

&

Who Is Ira Remsen

Objectives:

Define chemistry.

Identify possible clues that a chemical

change has taken place.

Relate pure chemistry to applied chemistry.

Chemistry is the study of matter and the changes

that it can undergo.

Matter is anything that has mass and occupies

space.

Chemistry is something that can be observed.

In lab, how will you know if matter is changed,

(if a chemical reaction occurs)?

An observation is the act of making and recording

a measurement. There are two types of

observations:

Qualitative data describes a non-number observation

(Quality)

Quantitative data describes number observations

(Quantity)

Label each data as qualitative or quantitative A beaker weighs 6.6 g, Sugar crystals are white & shiny,

Strontium fireworks burn red, the beaker gets hot

Write down as many observations that you can make

during the reaction of copper in nitric acid.

Evidence of a Chemical Reaction

Color change

Gas bubbles

Heat (exothermic)

Cooling (endothermic)

Flames/Light

Precipitate (ppt)

New odor

Types of Reactions:Precipitation (ppt) Exothermic & Light

Compare your observations to those of Ira Remsens

Ira was a well known Chemist (1846-1927) and Co-

discoverer of saccharin (Sweet N Low), He founded the

chemistry department at Johns Hopkins University

He is also famous for his story of watching nitric acid

acting upon copper while waiting in a doctors office.

http://www.eagan.k12.mn.us/fletcher/acn/flash/nitric_copper.html

http://www.eagan.k12.mn.us/fletcher/acn/flash/nitric_copper.html

Color change

Gas bubbles

Heat (exothermic)


Flames/Light

Precipitate (ppt)

New odor

As you listen to the Ira Remsen story, place

check marks next to the chemical changes that

you observe.

Ira Remsen:

Copper & Nitric Acid

Chemistry Areas of Study

Chemistry affects all aspects of life because living

and nonliving things are made of matter.

Some chemists enjoy doing research simply to

pursue chemical knowledge for its own sake. This

type of research is called pure chemistry, (the

chemist doesnt expect that there will be any

immediate practical use for the knowledge).

Ira Remsen was a chemist who enjoyed pursuing

pure chemistry

Most chemists do research that is designed to

answer a specific question this is known as

Applied chemistry. This research is directed

toward a practical goal or application. In practice,

pure chemistry and applied chemistry are often

linked.

Remember, Ira was a great observer, this is how

his laboratory discovered Saccharine (SweetN

Low).

Saccharine is Latin for sugary.

Ira & Discovery Of Saccharin

Cornell Question Guide

Explain why chemistry affects all aspects of

life.

Who is Ira Remsen and what discovery did

he make that we use in every day life?

How are chemistry and matter related.

Name 3 type of chemical changes

(reactions) that we will look for during an

experiment.

Bell Ringer:

Define Chemistry

List 3 types of observations indicating that

chemistry is occurring:

1.

2.

3.

Ch 1.1 and 1.2

What Is Chemistry?

Ch 1.3

Scientific Methods

Objectives:

Define chemistry.

Identify possible clues that a chemical

change has taken place.

Identify the steps of the scientific method.

Chemistry is the study of matter and the changes

that it can undergo.

Matter is anything that has mass and occupies

space.

Chemistry is something that can be observed.

In lab, how will you know if matter is changed,

(if a chemical reaction occurs)?

Evidence of a Chemical Reaction

Color change

Gas bubbles

Heat (exothermic)


Flames/Light

Precipitate (ppt)

New odor

Types of Reactions:Precipitation (ppt) Exothermic & Light

Ch 1.3

Scientific Methods

Scientific Methods Scientific methods are used by scientists to answer

questions and solve problems.

Below is a general process, not a checklist. A

scientist can begin investigating at any step within

the process but must describe their methods. That is

the purpose for a lab report.

Observations Observing The first step toward scientific discovery often

takes place when a scientist observes something no one has noticed before.

Qualitative data describes an observation (Quality)

Quantitative data use numbers (Quantity)

Label each data as qualitative or quantitative:

A beaker weighs 6.6 g, Sugar crystals are white & shiny, Fireworks are colorful

Hypothesis

Making a hypothesis: A hypothesis is a testable

explanation or answer to a question.

Experiments

A Hypothesis is meaningless unless there's data to support it.

Experiment is a set of controlled observations that test the

hypothesis.

One or more experiments are carefully planned in order to

change/test one variable at a time. Variables are quantities

that can have more than one value. There are 2 types of

variables:

Independent variable is that which you plan to change.

Dependent variables change in response to a change in the

independent variable.

Conclusion

Collecting data: Investigations and experiments

test a hypothesis. Data must be thoroughly

analyzed to determine whether the hypothesis was

supported or disproved. From the results, a

conclusion can be formed.

Publishing

Publishing results: Results of an investigation

are useful only if they are made available to other

scientists for a peer review. Many scientists

published their observations in scientific

literature.

Scientists will analyze the procedure, examine

the evidence, identify faulty reasoning, point out

statements that go beyond the evidence, and

suggest alternative explanations for the same

observations.

Forming a theory: A theory is a hypothesis that is

supported by a large body of scientific evidence over time.

Revising a theory: A theory is a hypothesis supported by

many experiments, but still subject to changes.

Scientific Law is the summary of accepted facts of nature.

Theory and Scientific Law

Cornell Guide

Chapter 1.3

Why should a hypothesis be developed

before experiments take place?

Give 2 qualitative and 2 quantitative data

types.

Name the 2 types of variables.

What is the difference between a theory and

a scientific law?

Reaction In A BagGo To

OneNote

How To Use Clickers

To turn on/off.

You will have to enter the

Version of your exam.

If you are A Version enter:

1 A

If you are B Version enter:

2 B

To Delete an answer.

To Scroll through

answers.

To Enter an answer.

Ch 2.3 & 3.4 (Glencoe)

Elements & Compounds

Objectives

Explain the difference between an element

and a compound.

Identify the chemical symbols of elements,

and name elements.

Ch 2.3 & 3.4 (Glencoe)

Elements & Compounds

Do you see Chemistry in this picture? Most people

say no, they dont. Chemistry cant be seen.

Therefore, Scientists represent atoms by using

different colored circles, called a model.

Models are tools that scientists use.

Cornell Questions?

What is the difference between matter,

atoms, and elements?

Matter is composed of tiny particles called

atoms.

Substances which cannot be broken down into

simpler substances by chemical reactions are

called atoms.

Not all atoms are alike, all matter is composed of

about 100 different types of atoms called

elements.

Each element is unique. Elements have their own

physical and chemical characteristics.

Below is an example of each element in model

format. An element in model form is a single,

colored circle.

Elements are organized in a table called the periodic

table of the elements

An element is identified by

its symbol; this consists of

one or two letters, usually

derived from its name:

C = Carbon

Co = Cobalt

Sometimes the element

symbol does not match the

element name. This occurs

because the Latin name is

sometimes used, i.e.

Cu = Copper (Cuprum)

If you look at the table below, other languages

(other than Latin) are used for element symbols.

Cornell Question?

What is the most important tool that a

scientist uses?

(Watch the video)

Cornell Questions?

How is each element different from

eachother?

How are the elements created?

How are the elements heavier than iron

(Fe) created?

(Watch the video)

Each element is

different from other

elements because it

has a different number

of protons.

As a result each

element has unique

physical & chemical

properties.

Elements are organized in the periodic table by the Blue

Number called the atomic number.

The atomic number is the number of protons in the

element.

Question#1: What is the symbol of the element

phosphorus & number of protons?

Question#2: What is the symbol of the element potassium

& number of protons?

Question#3: What is the symbol of the element Krypton 7

number of protons?

How Is The

Periodic Table Organized?

Take Out Blank Periodic Table

Label Groups

Going From Top To Bottom

Groups/Families

Elements with similar

chemical and physical

properties are in the

same column

Columns are called

groups or families

Label Periods

Going From Left To Right

Rows are called periods

Each period shows the pattern of properties repeated in the next period

Period 1

Period 2

Period 3

Period 4

Period 5

Period 6

Period 7

Metals, Metalloids, Nonmetals

Metallic Character

Metals Metalloids Nonmetals

Malleable & ductile

Shiny, lustrous

Also known as semi-

metals

Brittle in solid state

Good conductors of heat

and electricity

Show some metal and

some nonmetal properties

Poor conductors of heat

and electricity

(insulators)

Cornell Questions?

Weve been discussing how elements have

different physical and chemical properties.

(Watch the video)

List 3 physical properties:

List 3 chemical properties:

Physical & Chemical Changes

Cornell Guide

Chapter 2.3

Explain how an element symbol is represented.

Write the chemical symbol for each element:

Hydrogen, silver, helium, oxygen, gold

Name the chemical elements:

Cl, Fe, B, Be, Br

What is the difference between an atom and

element?

Practice: Protons & Elements

Practice: Element Name Word Search

Ch 3.4 (Glencoe)

Pure SubstancesObjectives:

Categorize a sample of matter as a substance or

a mixture.

Ch 3.4 (Glencoe)

Pure Substances DIVIDE YOUR CORNELL NOTES PAGE

INTO 3 COLUMNS

Elements Compounds Mixtures

Review:

Elements

Each element is unique. Elements have their own

physical and chemical characteristics.

Below is an example of each element in model format.

An element in model form is a single, colored circle.

A model is a visual of experimental data. Chemists use

models to represent matter, such as elements

Pure substances have fixed

properties:

Fe is a metal and magnetic

S is a nonmetal and not

magnetic

Elements are pure substances

Elements At

The Atomic

Level

Pure substances have a fixed

constant composition.

Elements are all the same,

thus a pure substance.

http://www.privatehand.com/flash/elements.html

The Element Song

http://www.privatehand.com/flash/elements.html

Polyatomic Elements

Poly (many) atomic (atoms) Polyatomicelements consist of several like atoms naturally bonded together

Memorize these 7 Diatomic elements:

H2, N2 , O2, F2, Cl2 Br2, I2

Remember

7th Heaven Rule

On Your Periodic Table

Color Code Those 7 Elements

Diatomic Elements

At The Atomic Level

Diatomic elements are pure substances

Compounds

Most substances are chemical combinations of

elements called compounds.

Below are some models of different compounds.

Compounds are more than one colored circle

connected by a stick known as a bond.

Compounds

Are Pure Substances

Compounds At The

Atomic Level

Compounds also have fixed

compositions, thus compounds

are pure substances.

Compounds are formed by a

chemical process.

The new compound has new

properties different from the

original elements that formed it.

Cornell Questions

1. Define pure substance:

2. List 3 examples of a pure substance:

3. Is carbon dioxide (CO2) a pure substance?

4. Explain why or why not:

Cornell Qs Continued

5. Define element:

6. Define compound:

7. How is it possible to distinguish an element from

a compound?

8. Name the elements contained in the following

compounds:

a. sodium chloride (NaCl) =

b. ethanol (C2H6O) =

c. ammonia (NH3) =

d. bromine (Br2) =

Complete Practice Problems:

Protons, Elements, Compounds, Mixtures

Only complete the first page

Review

Elements are organized in the periodic table by the Blue

Number called the atomic number.

The atomic number is the number of protons in the

element.

What are the models below?

Compounds or elements?

Pure substances or mixtures?

Ch 3.4 (Glencoe)

Mixtures

A mixtures is composed of two

or more pure substances

physically combined

Mixtures are separated by a

Physical process

In this case Fe and S are mixed

and separated physically with a

magnet

Mixture At The Atomic Level

Cornell Questions?

What is the color of the elements:

Iron (Fe) Fillings:

Sulfur (S) Powder:

How was the mixture of Iron and sulfur

physically separated?

How does one know if iron and sulfur had reacted

chemically instead of physically mixed?

Mixtures & Compounds Review

Cornell Questions

A)Element B)Compound

C)Mixture D) Pure Substance

________________

________________

________________

A)Element B)Compound

C)Mixture D) Pure Substance

_________________

_________________

_________________

Practice Problems To Complete:

Models of Elements, Compounds, &

Mixtures

3.4

Formulas of Elements &

Compounds

Objective:

Chemical symbols make it easy to write the

formulas of chemical compounds.

Review

Review: What are the models below?

Diatomic elements, compounds, or elements?

Name the atomic model below:

Element, Diatomic Element or Compound

Then classify:

Pure Substance or Mixture

________________

________________

________________

Instead of drawing models to represent

elements and compounds, it is more practical

to use the element symbols.

Formulas can be a single element or a

combination of element symbols to represent a

compound.

Note the next slide

1. H2

2. Mg

3. CO

4. Co

5. CO2

Are the formulas provided elements, compounds, or diatomic

elements?

If an element, write the name.

If compounds determine the number of elements in each compound

If diatomic element state diatomic element.

Answer

The answers are

Diatomic Element: H = 2

Element: Magnesium

Compound: C = 1 O = 1

Element: Cobalt

1. H2

2. Mg

3. CO

4. Co

5. CO2 Compound: C = 1 O = 2

Question

1. (NH4)2SO4

2. Na3PO4

3. Fe(NO2)3

4. CH3COOH

These formulas are compounds.

Determine the number of elements in each compound.

Answer

1. (NH4)2SO4 N = 2 H = 8 S = 1 O =4

2. Na3PO4

4. Fe(NO2)3

5. CH3COOH

Answers Are The Following:

1. (NH4)2SO4 N = 2 H = 8 S = 1 O =4

2. Na3PO4 Na = 3 P = 1 O = 4

4. Fe(NO2)3

5. CH3COOH


1. (NH4)2SO4 N = 2 H = 8 S = 1 O =4

2. Na3PO4 Na = 3 P = 1 O = 4

4. Fe(NO2)3 Fe = 1 N = 3 O = 6

5. CH3COOH


1. (NH4)2SO4 N = 2 H = 8 S = 1 O =4

2. Na3PO4 Na = 3 P = 1 O = 4

4. Fe(NO2)3 Fe = 1 N = 3 O = 6

5. CH3COOH C = 2 H= 4 O = 2


Element Compound or Diatomic Element?

Na

Na2O Element: Name of Element

NaHCO3

CaO

Ca(HCO3)2 Compound: Elements In Formula

Al

Al2O3

Al(HCO3)3 Diatomic Element

H2

O2


Element, Diatomic, Compound

Ch 10.3

Calculating amu

Objective:

Describe how to calculate the amu of a

compound.

Calculating AMU

Next, lets determine the mass of each atom.

As we learned, there are different types of

atoms known as elements.

Each element has a different mass and it is

called its amu

atomic mass units

Another name for amu is molar mass (Ch 6.4)

or molecular weight.

Molar mass is obtained by summing the masses

of the component atoms.

The amu is the red number in your periodic table

Amu is also known as its atomic weight

To calculate amu, go to 2 decimal placesLets look at a few

Go to 2 decimal places for AMU, lets look at a few:

N = O = K =

H = F = C =

Na = Li = Cl =

1. (NH4)2SO4 N = 2 H = 8 S = 1 O =4

2. Na3PO4 Na = 3 P = 1 O = 4

3. Fe(NO2)3 Fe = 1 N = 3 O = 6

4. CH3COOH C = 2 H= 4 O = 2

Remember This???

How Would We Determine The

amu Of CO2?First determine the number of atoms in the formula:

C =

O =


amu Of CO2First determine the number of elements in the formula:

C = 1 atom

O = 2 atoms

Next, find the amu for each element

(go to 2 decimal places):

C = 1 atom x 12.01 amu

O = 2 atoms x 16.00 amu

Finally, multiply the number of atoms by amu

And find the total amu:

C = 1 atom x 12.01 amu = 12.01 amu

O = 2 atoms x 16.00 amu = 32.00 amu



C = 1 atom x 12.01 amu = 12.01 amu

O = 2 atoms x 16.00 amu = 32.00 amu

CO2 total amu = 44.01 amu

How would we determine the amu of windex,

NH3?

Amu of NH3:

N = 1 atom

H = 3 atoms

Amu of NH3:

N = 1 atom x 14.01 amu

H = 3 atoms x 1.01 amu

Amu of NH3:

N = 1 atom x 14.01 amu = 14.01 amu

H = 3 atoms x 1.01 amu = 3.03 amu

Amu of NH3:

N = 1 atom x 14.01 amu = 14.01 amu

H = 3 atoms x 1.01 amu = 3.03 amu

total amu = 17.04 amu

or 17.04 molar mass

Lets practice another one

Calculate amu of butane:

C4H10


AMU Calculations ONLY pg. 2

Lab Partner Quiz

Name the atomic model below:

Element, Diatomic Element or Compound

Then classify:

Pure Substance or Mixture

________________

________________

________________

Go to 2 decimal places for AMU:

N = O = K =

1. (NH4)2SO4

2. Na3PO4

Calculate the AMU of the compounds below:

Ch 10.3

Percentage Composition

Using amu

Objective:

Describe how to calculate the percent

composition of an element in a compound.

How Can We Calculate

% Boys and % Girls In The Class?

To find percent of anything it is simply

this formula:

What You Want x 100%

The Total

What is the % Boys?

What is the % Girls?

Use amus for calculating Percentage Composition:

Percent composition = Element amu x 100%

Compound amu


%C and %O

First determine the number of atoms in the formula:

C =

O =

First determine the number of elements in the formula:

C = 1 atom

O = 2 atoms

Next, find the amu for each element

(go to 2 decimal places):

C = 1 atom x 12.01 amu

O = 2 atoms x 16.00 amu



C = 1 atom x 12.01 amu = 12.01 amu

O = 2 atoms x 16.00 amu = 32.00 amu


Compound amu

C = 1 atom x 12.01 amu = 12.01 amu/44.01 x100%

O = 2 atoms x 16.00 amu = 32.00 amu/44.01x 100%


% C = 27.29%

% O = 72.71%

(This adds up to 100%)

Look At Page 307:

What is the % N to % H of Windex, which is

NH3 (ammonia)?

Use amus for calculating Percentage Composition:


Compound amu

First determine the amu for the

formula NH3:

How would we determine the amu of windex,

NH3?

Amu of NH3:

N = 1 atom

H = 3 atoms

Amu of NH3:

N = 1 atom x 14.01 amu

H = 3 atoms x 1.01 amu

Amu of NH3:

N = 1 atom x 14.01 amu = 14.01 amu

H = 3 atoms x 1.01 amu = 3.03 amu

Amu of NH3:

N = 1 atom x 14.01 amu= 14.01/17.04 x 100%

H = 3 atoms x 1.01 amu =3.03/17.04 x 100%

total amu = 17.04 amu

% N = 82.22%

% H = 17.78%

(Adds up to 100%)

The percentages may not always total to 100% due to rounding,

for example if you go to 1 decimal spot

82.2% N

+ 17.7% H

99.9 % total

But if you go to 2 decimal spots you get closer to 100%

82.21% N

+ 17.79% H

100.00 % total

Overall your numbers should

add up close to 100%

Lets practice another one

Calculate Percentage composition of

butane C4H10:


% Using AMU

Ch 10.3

Calculating % Composition By

Given Masses

Objective:

Describe how to calculate the percent by

mass of an element in a compound.

Ch 10.3

Calculating % Composition By

Given Masses

The Law of Definite Proportions states that a

compound is always composed of the same

elements in the same proportion by mass.

The mass of the compound is equal to the sum of

all the masses of the elements.

Percent by mass:

% Composition = Part Element Mass x 100%

Total Compound Mass

A sample of butane (C4H10)--lighter fluid--

contains 288 g carbon and 60 g hydrogen.

Find %C and %H in butane

%C =

%H =

A sample of butane (C4H10)--lighter fluid

contains 288 g carbon and 60 g hydrogen.

First find the total

288 g C + 60 g H = 348 g

Part Part Total

Next, calculate the percent of each element:

Percent composition = Part x 100%

Total

288 g C + 60 g H = 348 g

Part Part Total

Can you figure it out?

Next, calculate the percent of each element:


Total

288 g C + 60 g H = 348 g

Part Part Total

288 g C (C part) x 100 % = 82.8 % C

348 g (Total)

60 g H (H part) x 100% = 17.2 % H

348 g (Total) + ---------------

100.0 %

Percents should add up close to 100%

Now you and your lab partner try this one

What is the percentage composition of

carbon and oxygen in a compound, that contains

40.8 g of carbon and 54.4 g of oxygen.

% C = ?

% O = ?

40.8 g of carbon + 54.4 g of Oxygen = 95.2 g total


Total

40.8 g of carbon x 100 % = 42.86% Carbon

95.2 g total

54.4 g of Oxygen x 100% = 57.14% Oxygen

95.2 g total


% Composition By Given Mass

Ch 2.3

Uncertainty In Data

Objective: Identify and apply measurement

techniques and consider possible effects of

measurement errors.

Ch 2.3

Uncertainty In Data

Accuracy

Accuracy refers to how close an experimental

measurement is to some accepted value

(theoretical value), well use % error:

(NOTE: Use Absolute Value)

% error = exp value accepted value x 100%

accepted value

In lab Josh finds the boiling point of rubbing

alcohol to be 75 degrees. He looks online at the

Handbook of Chemistry & Physics that the

boiling point should be 80. degrees.

Calculate the % Error:


accepted value

Jill weighs an element on a balance. The element

has a mass of 24.3 grams. The periodic table has

the accepted value to be 25.7 grams.



accepted value

The density of water at 4 degrees is 1.00 g/mL.

John experimentally found the density to be 1.08

g/mL.



accepted value

Ch 10.3

Calculating the AMU Of A

Hydrate Crystal

Objective:

Describe how to calculate the AMU of a

hydrate crystal.

Ch 10.3

Calculating the AMU Of A

Hydrate Crystal

Ch 10.3

Calculating the % Water Of A

Hydrate Crystal

Objective:

Describe how to calculate the percent water

of a hydrate crystal.

Ch 10.3

Calculating the % Water Of A

Hydrate Crystal

Lab Power Point

Hydrate Crystals

Title: % Water In A Hydrate

Purpose: Analysis of the % water of an unknown

crystal & to I.D. the hydrate from a list of

possible calculated unknowns.

Pre-Lab Notes:

Hydrate Definitions

Hydrates

A compound that is hydrated is called a hydratesince they form solids that include water in their crystal structure.

Compounds that contain water molecules as part of their

crystal structure are called hydrates.

Heating a hydrate drives off the water molecules, and

the solid that remains behind is called anhydrous,

meaning without water.

By simply heating the solid, water can be driven from a

hydrate to leave an anhydrous compound.

Notice the color difference of:

Anhydrous crystals copper (II) sulfate

NOTE: Black material is Copper II Oxide

Hydrate crystals copper (II) sulfate

Hydrate AMU Calculation

CuSO4 5 H2O

When calculating the molar mass

add the AMU of water. The dot

indicates 5 waters, therefore add

the salt AMU + water AMU

CuSO4 5 H2O

Calculate below:

% Water Calculation

Practice Obtaining

Acceptable Value

How to calculate Percentage Water:

% water = # of waters amu x 100%

hydrate crystals amu

% water = 5 H2O amu x 100%

CuSO4 5 H2O amu

Practice Problems:

AMU of Hydrates

Use AMU of Hydrates to practice

calculating % water in each hydrate

crystal

Practice Calculating % Water: Cd(NO3)2 4 H2O

NaClO4 1 H2O

Ba(OH)2 8 H2O

NiCl2 6 H2O

Practice Obtaining Experimental

Values

When you find the mass

of substances that you

heat, you have to weigh

the containerWhy

should one do this?

Calculate % Water

experimentally using

the next slide and

video

Lets copy the sample data tables below (were still in pre-

lab notes of the lab)

#1 Mass empty crucible: ____________________________

#2 Mass crucible+hydrate salt (before heating): __________

#3 Mass of crucible+anhydrate (after heating): __________

Lets watch the experiment:

#1 Mass empty crucible:

#2 Mass crucible+hydrate salt (before heating):

#3 Mass of crucible+anhydrate (after heating):

#1 Mass empty crucible: 20.057 g

#2 Mass crucible+hydrate salt (before heating): 45.551 g

#3 Mass of test tube+anhydrate (after heating): 38.547 g

Copy the data tables below and calculate (show work):

Calculate the mass of the hydrate (#2 - #1):

Calculate the mass of water lost during heating (#2 - #3):

Calculate % water in the hydrate (Experimental Number);

g water x 100%

g hydrate crystal

#1 Mass empty crucible: 20.057 g

#2 Mass crucible+hydrate salt (before heating): 45.551 g

#3 Mass of test tube+anhydrate (after heating): 38.547 g

Calculate the mass of the hydrate (#2 - #1):

45.551 g

- 20.057 g

25.494 g Blue Hydrate Salt

Calculate the mass of water lost during heating (#2 - #3):

45.551 g

- 38.547 g

7.004 g of Water Lost

Calculate the percent water in the hydrate g of water x 100% =

g of Hydrate Salt

7.004 g of Water Lost X 100% = 27.47% Water

25.494 g Blue Hydrate Salt Experimental Value

How Would You Calculate

% Error??

Accepted value (theoretical value calculated on

paper using the periodic table).

Experimental value is found from data in the lab.


accepted value

check next slide

Accepted % Water (using periodic table):

90.10 g water x 100% = 36.08 %

249.72 g Hydrate accepted value


accepted value

Experimental % Water (using data):7.004 g of Water Lost X 100% = 27.47% Water

25.494 g Blue Hydrate Salt Experimental Value

Procedure: (Use OneNote PDF)

Review How To Use

An Electric Balance

Practice Problems:

AMU of Hydrates

Use AMU of Hydrates to practice

calculating % water in each hydrate

crystal

Practice Calculating % Water: Cd(NO3)2 4 H2O

NaClO4 1 H2O

Ba(OH)2 8 H2O

NiCl2 6 H2O

Ch 2.3

Uncertainty In Data

Objective: Identify and apply measurement

techniques and consider possible effects of

measurement errors.

Accuracy

Accuracy refers to how close an experimental

measurement is to some accepted value

(theoretical value), well use % error:


accepted value

In lab Josh finds the boiling point of rubbing

alcohol to be 75 degrees. He looks online & the

boiling point should be 80 degrees.



accepted value

Jill weighs an element on a balance. The element

has a mass of 24.3 grams. The periodic table has

the accepted value to be 25.7 grams.



accepted value

The density of water at 4 degrees is 1.00 g/mL.

John experimentally found the density to be 1.08

g/mL.



accepted value

If you remember Accuracy refers to how close

an experimental measurement is to some

accepted value (theoretical value), well use %

error:


accepted value

CuSO4 5 H2O Recently we calculated the amu ofCopper II Sulfate PentaHydrate

theoretically the amu is the

following:

CuSO4 5 H2O amu = 249.69

CuSO4 5 H2O Calculate % Water theoretically using the amu:

CuSO4 5 H2O amu = 249.69

90.10 g water x 100% = 36.08 %

249.69 g Hydrate accepted value

Chemical Changes

Chemical reactions are chemical changes. It involves

the rearrangement of atoms to produce new substances

and chemical changes.

How do we know if matter is

changing (chemistry occurring)?

Observations to watch for:

Permanent new state change (e.g. liquids to solid, ppt)

Formation of gas bubbles

Formation of light or flames

Temperature change (e.g. gets colder or hotter)

A color change

A new odor

The first video will

illustrate how O2 gas

and H2 react to form

water (chemical

reaction)

The second video will

show how we can use

this type of reactions

energy as a fuel

source for the Space

Shuttle

The

Law Of Conservation

The Law of Conservation of Mass states that atoms are neither created nor destroyed

Atoms are merely rearranged to create something new, with new chemical and physical properties

Lets observe the reaction movie on the next

slide.

Is the law of conservation of mass shown?

Note the beakers before and after

Id say the law of conservation of mass is shown

Parts Of A Chemical Equation

Reactants are the chemicals reacting

Products are the chemicals produced

Use the + sign to separate chemicals

Use the yield sign

(Do NOT Use = equals sign)

To obey the Law of Conservation it must be balanced by adding coefficients mass of reactants = mass of products

We will learn to balance equations later.

Ch 2.2

Changes In Matter

Objective:

Three states of matter are solid, liquid, and gas

Matter is the part of the universe that has mass

and volume and exists in three phases:

Solid

Liquid

Gas

Phase changes

are NOT

chemical changes!

Solid:

Does not flow easily

Definite (fixed) shape

Definite (fixed) volume

Particles are close together

(thus not easily compressible)

Liquid:

Flows easily.

Definite shape (takes the shape

of any container)

Definite volume

Little space between particles

(thus not easily compressible)

Gas:

Flows easily

Takes the shape of the

container

Fills the volume of the

container

Particles are very far apart

(thus, easily compressible)

Physical Changes

Physical Changes The process of boiling and freezing causes

physical changes. I.g.

water changes form but

still remains the H2O

compound.

The change is in the

form of a substance &

not its chemical

composition.

H2O (s) = solid water

H2O (l) = liquid water

H2O (g) = gas water

(water vapor)

2.2

Mixtures Of Matter

There are two types of mixtures

Mixtures can be Homogeneous or

Heterogeneous

Homogeneous Mixtures

Homogeneous mixtures (a uniform

mixture) has a composition that is the

same throughout. It is also known as a

solution.

The solute is usually the

smaller number and it gets

dissolved

The solvent is usually the

bigger number and does

the dissolving

The homogeneous

mixture, the solution

consists of the solute and

solvent thoroughly mixed.

Solute + Solvent = Solution

2.18 g

Solute

55.50 g

Solvent

Solution

Remember:

Solute + Solvent = Solution

To finding % mass in solution:

Solute mass x 100%

Solution mass

2.18 g

Solute

+ 55.50 g

Solvent__

57.68g2.18 g x 100%

2.18 g +55.50g

2.18 g x 100% = 3.78%

57.68 g

The next video segment will show how a

solution is made

Types of Solutions

Solutions dont have to be a solid solute dissolved

in an liquid solvent.

Gaseous solutions:

For example Air =

80% N2 and 20% O2

Solid Solutions:

For example door knobs =

67% Cu and 33 % Zn

Solutions which consist of a gas solute dissolved

in a liquid solvent:

carbonated drinks =

CO2 and H2O

Video Review: Solutions

Heterogeneous Mixtures

Heterogeneous mixtures (are non-uniform mixtures)

they have different composition and properties and

several components can be distinguished from one

another

This usually occurs when a solute is not soluble in a

solvent.

Separation of Mixtures

Separation of Mixtures

Many different methods can be used to separate

the components of a mixture from one another

This involves a physical change

NO chemical reaction is needed, substances are

NOT bonded, just physically combined

Here are a couple of methods that you may carry

out in the laboratory

Decanting separates a liquid from a solid

Filtration separates a liquid from a solid as well

For example, filtering sand from saltwater

Distillation Distillation:

separates a solution

by different boiling

points

Water is separated

from the salt by

heating the solution,

minerals are left

behind and the

steam is condensed

to pure water.

This is how distilled

water is made

http://adventure.howstuffworks.com/27665-g-

word-water-desalination-video.htm

Watch this video segment about distilling

dirty water to produce clean water

http://adventure.howstuffworks.com/27665-g-word-water-desalination-video.htm

Paper Chromatography Chromatography:

separates a solution of

different colors

Here a strip of porous

paper, such as filter

paper, is dipped into a

liquid, which travels

up the paper, like a

wick, and the ink

mixture separates into

its component colors

For chromatography the

solute is the dye and the

solvent is the water.

You need to make sure

that the solute and

solvent are chemically

similar so that the

process of

chromatography will

work This is called

solubility

Review: Separating Mixtures

Documents

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