Topic 1.1 Matter & Change

EI: physical and chemical properties depend on the ways in which different atoms combine.

NOS: Making quantitative measurements with replicates to ensure reliability – definite and multiple proportions (3.1)

What is Matter?

What is Matter?

•Anything that takes up space and has mass.

– Made up of particles (atoms, molecules, ions)– Particles are in constant motion

A 2. States of Matter

State Shape VolumeDistance between particles

Arrangement of particles

Solid (S)

Fixed shape

Fixed volume

Close together regular

Liquid (l)

No fixed shape

Fixed volume

Close, but farther than solids

random

Gas or Vapor

(g)

No fixed shape

Not fixed Far apart random

Switching between states

• Solid melting Liquid

• Liquid freezing Solid

• Liquid evaporating (boiling) Gas

• Gas condensing Liquid

Switching between states

• Solid sublimation Gas

• Gas deposition Solid

Heat is required from solid to liquid to gas

Heat is removed from gas to liquid to solid

Switching between States

U1: Properties of Matter

Physical property• A characteristic of a substance

that can be measured or observed without changing the substance’s composition

Chemical property• The ability of a substance to

undergo a chemical reaction to form new substances

U1. Properties of Matter

Examples of Physical Properties

• Color• Solubility (Dissolving)• Odor• Hardness • Density• Melting Point• Boiling Point• State of matter• Thermal capacity• Mass

Examples of Chemical Properties

• Reactivity with oxygen • Reactivity with acids• Reactivity with bases• Reactivity with other

elements

Sodium and Chlorine Reaction

U1. Properties of Matter

Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC.

• Using the above description, list the physical properties of sodium

• Using the above description, list the chemical properties of sodium

U1. Properties of Matter

Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC.

• Using the above description, list the physical properties of sodium

• Using the above description, list the chemical properties of sodium

U1. Changes of Matter

Physical change• An alteration of matter that

does not change the chemical composition of the material.

U1. Changes of Matter

.

Chemical change• Results in a change in the

chemical composition of the substance(s). This is called a reaction.

U1. Changes of Matter

Examples of Physical Changes

• Freezing or melting• Boiling or condensing• Cutting• Grinding • Bending• Blending• Dissolving

Examples of Chemical Changes

• Combustion (burning)• Reacts with an acid• Reacts with a base• Rusting• Oxidizing• Decomposing• Digesting

U1. Changes of Matter Copy the statement on your paper and write P for

physical or C for chemical

1. Bending of a piece of wire

2. Burning of coal

3. Cooking a steak

4. Cutting grass

5. Sodium reacts with water

6. Iron rusts7. Silicon is insoluble in

water8. Ice melts9. Neon boils at -2460C10. Nitric Acid reacts

with Copper

U2. Distinguishing Compounds and Mixtures

• Elements are composed of just one type of atom. They cannot be separated into simpler substances using chemical means.

U2. Distinguishing Compounds and Mixtures

• Compounds are substances composed of two or more different kinds of atoms that have combined chemically. They can be separated by chemical means.

U2. Distinguishing Compounds and Mixtures

• Mixtures are a physical blend of two or more substances. They can be separated by physical means.

U2. Distinguish compounds and mixtures

• Elements– Represented by a chemical symbol (see Periodic

Table)

– Gold (Au), Iron (Fe), Oxygen (O or O2)

U2. Distinguish compounds and mixtures

Compounds– A fixed ratio of elements,

shown using element symbols and a number

U2. Distinguish compounds and mixtures

• Compounds– Examples:

• Water, H2O, contains 2 atoms of hydrogen (H) and one atom of oxygen(O).

• Salt, NaCl, contains one atom of sodium (Na) for each atom of chlorine (Cl).

U3. Mixtures

Mixtures: composition is not fixed• Homogeneous mixture- has uniform

composition and properties, also called solutions.– Ex: pure air, pure water, syrup

U3. Mixtures

Mixtures:• Heterogeneous mixture – non-uniform

composition, properties are not the same, able to see the separate components

• Ex: soup, concrete, granite

U3. Mixtures

• Ways to separate mixtures:– Heterogeneous: sieving, tweezers, skimming

– Homogeneous: distillation, ion exchange, reverse osmosis, evaporation

Distinguish between elements, compounds, and mixtures

Copy the item and indicate if it is an element, compound or mixture

1. Blood2. Hydrogen3. Brass (copper and zinc)

4. Ice (H2O)5. Motor oil

6. Silver

7. Orange juice

8. Neon

9. Sugar (C6H12O6)

10. Lake water

A& S. 1: Chemical Reactions

• In a chemical reaction, one or more substances change into new substances by rearranging the atoms

• Reactants Products

A& S. 1: Chemical Reactions

•Reactants ProductsReactants: the substances that are combined together

Products: the substances that are formed after the reactants are combined together.

A& S. 1: Chemical Reactions

Chemical Reaction Example:•Reactants Products

Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water

Cu + HNO3 Cu(NO3)2 + NO2 + H2O

A& S. 1: Chemical Reactions

•Reactants Products

Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water

Cu + HNO3 Cu(NO3)2 + NO2 + H2O

A&S 1. Chemical Reactions

A chemical reaction has occurred if:– Heat is absorbed or given off (change in

temperature)– Change in color or odor– Production of a gas or solid– Not easily reversible

A&S 1. Chemical Reactions

Law of Conservation of MassDuring any chemical reaction, mass is neither created nor destroyed, it is conserved.

– The mass of the products will always equal the mass of the reactants.

– The mass of each element is also unchanged.

A&S 1. Chemical Reactions

Law of Conservation of MassIn a reaction where hydrogen reacted with oxygen to produce water, if 4.5 g of hydrogen and 34 g of oxygen were used, how many grams of water were produced?

Hydrogen + oxygen = water4.5 + 34 = 38.5 g water