Name: ___________________________________________________________________ Period: __________

CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW

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Unit 1: Nature of Science Essential questions:

What rules must be obeyed to safely conduct an experiment?

What are the components of a good scientific experiment?

What rules must be obeyed to safely conduct an experiment?

Why are significant figures important to chemists?

What is the best method/graph to represent specific data?

How would a scientist organize data collected from an experiment into a graph?

How does a standard notation number compare to a scientific notation number?

How do you differentiate between accuracy and precision of data?

Can you calculate % error of the results from an experiment?

What are the SI base units?

How is dimensional analysis used to convert units within the metric system?

Why does the Big Bang Theory exist?

Explain scientifically behind how the universe was created according to the Big Bang Theory? Key vocabulary:

Scientific method

Significant figures

Metric system

Base units

Big Bang Theory

Experiment

Hypothesis

Variable

Control

Accuracy

Precision

Percent error Practice:

1. Using the picture to the right, list lab safety rules that are being ignored.

2. What are the steps to the scientific method?

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3. Convert the following into scientific notation:

a) 1500 = ____________ c) 0.001012 = ____________

b) 123 = ____________ d) 1.52 = ____________

4. Convert the following into decimal notation (ordinary notation):

a) 4.59 x 103 = ____________ c) 280 x 10

-4 = ____________

b) 5 x 102 = ____________ d) 1.4 x 10

-5 = ____________

5. Indicate the number of significant figures:

a) 34 g ___ b) 564 L ___ c) 19.3 mm ___

d) 23.45 mg ___ e) 101 km ___ f) 3400 g ___

6. Round the following numbers to 2 significant figures:

a) 0.826mg ___ b) 19.88mL ___ c) 19250cm ___ d)950L ___

7. What is the SI unit for the following measurements:

a) length _____ b) mass _____ c) time _____ d) volume _____

8. What measurement in millimeters is indicated on the ruler below? _____

9. Convert the following:

a) 850cm to mm b) 2500 mg to kg c) 0.2598kL to L

10. Suppose a lab refrigerator should hold a constant temperature of 38.0 F. A temperature sensor is tested 10 times in the

refrigerator. The temperatures from the test yield the temperatures of: 37.8, 38.3, 38.1, 38.0, 37.6, 38.2, 38.0, 38.0, 37.4, 38.3.

Is the distribution of values from the test: accurate (yes or no), precise (yes or no). Why?

11. Explain the Big Bang Theory. _________________________________________________________________________________

________________________________________________________________________________________________________

________________________________________________________________________________________________________

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12. What is the equation for percent error?

13. A researcher measures the mass of a sample to be 5.51 g. The actual mass of the sample is known to be 5.80g. Calculate the percent error.

Unit 2: Atomic Structure Essential questions:

What is an atom?

What are the early models of the atom and how has scientific exploration lead to the current model?

What is a theory?

How do you identify the relative mass, relative charge, and location of the three smaller subatomic particles of an atom?

What is the overall charge of an atom?

What is the relationship between the subatomic particles and their charges, masses, and locations?

What is an isotope?

What is the average atomic mass compared to atomic mass?

How do you calculate the average atomic mass of elements?

Identity an element when supplied with the natural abundance and mass of each isotope.

Key vocabulary:

Atom

Compound

Subatomic Particles

Proton

Neutron

Electron

Nucleus

Atomic Number

Average Atomic Mass

Mass Number

Isotope

Neutral

Theory

Practice: 14. What is an atom? _________________________________________________________________________________________

15. What is the overall charge of an atom? Why? ___________________________________________________________________

________________________________________________________________________________________________________

16. Circle the correct option: Isotopes are atoms of the same element, which have the same number of (protons / neutrons) but a

different number (protons / neutrons).

17. How do isotopes C-12 and C-14 differ from each other? ___________________________________________________________

How are they similar? ______________________________________________________________________________________

18. What parts of Dalton’s atomic theory are now known to be incorrect? _______________________________________________

________________________________________________________________________________________________________

________________________________________________________________________________________________________

________________________________________________________________________________________________________

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19. Progression of the atomic model:

Dalton Thompson Rutherford

Description of

supporting

evidence &

experiments

Major findings

Drawing and

description of

atomic model

20. Identify the three basic particles in the atom. Give their location, charge, and mass. (Fill in the table)

Particle Location Charge Mass (amu)

21. Fill in the blanks for the elements using the periodic table

Element Symbol Atomic # #Protons # Electrons #Neutrons Mass #

Carbon-14

29 35

16 32

131

53 I

47 108

22. Silicon has three naturally occurring isotopes. Calculate the average atomic mass of Silicon with the information provided. Check

your answer using the periodic table.

Isotope name Isotope mass (amu) Relative Abundance

Silicon-28 27.98 92.21

Silicon-29 28.98 4.70

Silicon-30 29.97 3.09

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Unit 3: Electron

Essential questions:

How does an electron act according to de Broglie’s wave-particle duality?

What is a quantum?

In what ways do the Bohr model and quantum mechanical model differ?

How does the quantum mechanical model describe the arrangement of the electrons in atoms and their orbitals?

What happens when electrons in atoms absorb or release energy?

How is the electron arrangement of an atom indicated by electron configurations and orbital diagrams?

How are electron configurations different from noble gas configurations?

How is atomic emission spectra of elements used to identify elements?

What is the relationship between a wave’s frequency, energy, and wavelength?

Key vocabulary:

Wave-Particle Duality

Electron

Excited State

Ground State

Quantum

Valance Electron

Frequency

Energy

Wavelength

Electron Configuration

Noble Gas Configuration

Electromagnetic Spectrum

Orbitals

Period

Energy Level

Cloud Shapes

Practice:

23. Electrons can act as a __________ or ___________ according to the _____ -__________ duality model.

24. What is a quantum of energy? __________________________________________________________________

25. When an electron absorbs energy, it jumps to the ___________ state.

26. How does an electron produce light in things such as fireworks or neon signs? ______________________________

________________________________________________________________________________________

Use the diagram to answer questions 27-29:

27. Which region is referred to as the s-block on the diagram? ____

How many electrons can each level of the s-cloud hold? ____

28. Which region is referred to as the p-block on the diagram? ____

How many electrons can each level of the p-cloud hold? ____

29. Which region is referred to as the d-block on the diagram? ___ How many electrons can each level of the d-cloud hold? ___

30. What energy level are the outer electrons for potassium found? ______ This is indicated by potassium’s ______________.

31. Indentify the number of valance electrons for the following elements and draw the corresponding electron-dot structure:

a) Calcium b) Carbon c) Neon

32. Draw the shape of the s-sublevel: Draw the shape of the p-sublevel:

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33. Write the electron configuration for:

Lithium:

Argon:

Iron:

Barium:

34. Identify the element with the electron configuration of 1s22s

22p

63s

23p

3 ____________________

35. Identify the element with the electron configuration. [Ne]3s23p

4 _________

36. According to the quantum mechanical model, the location of an electron is based on ______________.

37. What does the electromagnetic spectrum show? _____________________________________________________________

_____________________________________________________________________________________________________

38. On the electromagnetic spectrum, as the wavelength increases, frequency ___________, and energy ____________.

39. A barium atom (gains / loses) ______ electrons when it forms a barium ion. What is the symbol for a barium ion? ______

A fluorine atom (gains / loses) ______ electrons when it forms a fluorine ion. What is the symbol for a fluorine ion? ______

40. Write the orbital notation for:

Carbon: Iron:

Unit 4: Periodic Table

Essential questions:

How is the periodic table organized according to Mendeleev and Moseley?

What information does the periodic table provide?

What property of elements is used to organize the periodic table?

How many groups and periods are on the periodic table?

What are the family names for groups 1,2,3-12, 17,18?

Where are the metals, nonmetals, and metalloids located?

How can periodic trends be explained?

Key vocabulary:

Atomic Number

Atomic Mass

Atomic Symbol

Group (family)

Period

Group Names

Metals

Nonmetals

Metalloids

Periodic trend

Atomic radius

Ionic Radius

Electronegativity

Octet Rule

Practice: Use the diagram to answer questions 41-43 :

41. Which region contains group 18? ___ What is the name of this group? ____________

42. Which region contains the alkaline earth metals? _____

43. Which region contains elements with an electron configuration that ends with p5? _____

44. The 10 short columns in the middle of the periodic table make up the ___________________ _________________.

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45. The order of the elements on the periodic table is based upon the ____________ ______________. What particle of the atom

is represented by this number? __________________

The diagram to the right lists the information found on the periodic table. Use this diagram to answer question 46.

46. The element’s ____________________ is 79, the _____________ is Au, and the Atomic mass is ____________.

47. How many groups are on the periodic table? ____________

48. How many periods are on the periodic table? ____________

Use the diagrams below to answer questions 49-50.

49. Which diagram correctly depicts the trend in electronegativity? ________

50. Which diagram correctly depicts the trend in atomic radius? ________

51. Elements in the same group have similar ______________________________. They behave similarly because they have the

same number of ________________.

52. Metals are located on the ____________ side of the periodic table and nonmetals are on the ____________ side.

79

Au

Gold

107.86

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Unit 5: Bonding

Essential questions:

How do intermolecular forces differ from intramolecular forces?

How is a positive and negative ion formed?

Why does an element gain or lose electrons to become and ion?

How do ionic compounds form?

How does covalent bonding satisfy the octet rule?

How is the bonding in Covalent (molecular) compounds different from the bonding in ionic compounds?

How do the properties of an ionic compound compare to those of covalent (molecular)compounds?

How many electrons are shared between atoms in a double and triple bond?

How do electrons affect the shape of a molecule?

How do lone pairs around a central atom affect the polarity of the molecule?

Why can carbon form many compounds?

Key vocabulary:

Ionic bond Ionic compound Covalent bond

Covalent compound

Valence Electron

Intramolecular forces

Intermolecular forces

Ions

Cation

Anion

Polarity

Single, double triple bond

Physical properties

VSEPR

Octet rule

Lone pairs

Practice: 53. How does a intermolecular forces differ from a intramolecular force? ________________________________________

_________________________________________________________________________________________________

54. Which electrons are involved in bonding? _________________________________

55. What types of elements are involved in ionic bonding? ________________________ Covalent?___________________

56. What type of bond is formed by the transferring of electrons? ________________ Sharing electrons? ______________

57. How does an element form a cation?______________________________ Anion? _____________________________

58. Why does Magnesium form a +2 charge? _______________________________________________________________

59. How many valance electrons does each of the following elements have?

a) Sodium ________ b) Oxygen __________ c) Krypton __________

60. List the general characteristics of ionic and covalent bonds (i.e. physical properties (hardness, state of matter, boiling point, melting point, conductivity), strength)

Ionic

Covalent

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61. Using electronegativity values, what type of bond (ionic, polar covalent, nonpolar covalent) is formed between the following elements (show calculation):

b) F and F b) H and I c) Mg and Br d) C and Cl

62. How many electrons are shared in a: c) Single covalent bond ___ b) Double covalent bond ___ c) Triple covalent bond ___

63. Why do some elements form double and triple bonds during bonding? ________________________________________

_________________________________________________________________________________________________

64. Draw Lewis structures for the following. Identify the shape of the molecules (linear, bent, tetrahedral, trigonal planar and pyramidal). Identify the polarity of the molecules.

Molecule E-Dot Structure Shape Molecular

Polarity

Molecule E-Dot Structure Shape Molecular

Polarity

H2O

BF3

NFH2

PH3

CF4

CO2

Unit 6: Chemical Nomenclature

Essential questions:

How are ionic compounds identified?

What is a monatomic ion?

What are the common polyatomic ions’ names and formulas?

How are cations and anions combined to make ionic formulas?

How are Roman numerals used in ionic compound formulas?

How do you identify ionic compounds versus covalent (molecular) compounds?

What are the diatomic elements?

How are molecular formulas translated into binary covalent compound names? Key vocabulary:

Ionic compound Polyatomic ions Nonmetals

Covalent compound

Valence Electron

Ions

Cation

Anion

metals

Transition Metals

Octet rule

Binary Compound

Diatomic Molecules

Subscript

Superscript Practice: 65. Identify all seven diatomic elements: ___________________________________________________

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66. Write the formulas and charges for the following polyatomic ions: hydroxide: sulfate: phosphate: ammonium: nitrate: carbonate: 67. For the following ionic names, write the missing chemical formula or chemical name.

a. nickel (II) oxide _____________ b. calcium carbonate _____________

c. potassium nitrate _____________ d. ammonium bromide _____________

e. gold (III) iodide _____________ f. zinc phosphide _____________

g. lithium sulfate _____________ h. Na2SO4 ___________________________

i. Al2O3 ___________________________ j. SnO ___________________________

k. K2S ___________________________ l. (NH4)3PO4 ___________________________

m. ZnCl2 ___________________________ n. PbCO3 ___________________________

68. For the following molecular (covalent) compounds write the missing formula or name.

a. carbon monoxide ____________ b. xenon tetrafluroide ____________

c. silicon dioxide ____________ d. iodine pentachloride ____________

e. P2O5 ___________________________ f. P4O10 ___________________________

g. SF7 ___________________________ h. NI3 ___________________________

Unit 7: The Mole

Essential questions:

How is the mole used to count particles of a substance?

How does the mole relate to other everyday counting units?

Why is the mole used to count atoms instead of a more common unit?

How are moles of a substance converting to numbers of representative particles?

How is molar mass of a substance calculated?

How is the mass of an atom related to the mass of a mole of atoms?

How are moles of a substance converted to mass?

How are number of representative particles of a substance determined from its mass?

What is the difference between an empirical and molecular formula of a compound?

How is the percent composition of an element within a compound calculated?

How are empirical and molecular formulas obtained from percent composition data? Key vocabulary:

Mole

Atoms

Avogadro’s Number

Representative Particle

Hydrate

Molar Mass

Empirical Formula

Molecular Formula

Subscript

Percent composition

Practice:

Show all work for calculations:

69. Give conversion factors (in fraction form) for converting between the following

A.) FROM moles TO atoms B.) FROM grams TO moles of Boron C.) FROM atoms TO moles

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70. What is the molar mass of Rb2Cr2O7?

71. What is the % by mass of C in Pb(C2H3O2)2 ?

72. What is the molar mass of CoCl2 6H2O ?

73. What is the number of molecules in 16.75 g of H2O ?

74. What is the mass of 1.75 x 1024 molecules of NH3 ?

75. How many molecules are in 0.26 mol of CO2 ?

76. Which of the following are empirical formulas? H2O H2O2 C6H12O6 N2H5

Unit 8: Chemical Reactions

Essential questions:

What is evidence of a chemical change?

How is a chemical change different from a physical change?

How does a balanced chemical equation show relationships between the reactants and the product of a chemical reaction?

How can chemical reactions be classified?

What are the defining characteristics of each classification of chemical reaction?

What are aqueous reactions?

How are word equations translated into formula equations and vice versa? Key vocabulary:

Chemical Change

Physical Change

Coefficient

Molar Ratio

Conservation of Matter

Balanced Reaction

Chemical Reaction

Synthesis

Decomposition

Single Replacement

Double Replacement

Combustion

Aqueous Solution

Precipitate

Practice:

77. Differentiate between a precipitate and an aqueous solution. ______________________________________________

____________________________________________________________________________________________

____________________________________________________________________________________________

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78. List the 5 types of chemical reactions AND state how you would identify their type simply by looking at the equation:

Type of reaction: How you would identify the type simply by looking at the form of the equation?

S = Synthesis (Combination) 2 or more reactants and only 1 product

D =

SR =

DR =

C =

79. Why do chemical equations need to be balanced? _______________________________________________________

____________________________________________________________________________________________

80. Balance the following equations and identify the type of reaction occurring:

a. ____Zn + ____HCl ---> _____ZnCl2 + ____H2 type ___________________________

b. _____KClO3 ---> _____KCl + ____O2 type ___________________________

c. ____S8 + ____F2 ---> _____SF6 type ___________________________

d. _____Fe + ____O2 ---> ____Fe2O3 type ___________________________

e. ____C2H6 + ____O2 ---> ____CO2 + ____H2O type ___________________________

f. _____MgO _____Mg + _____O2 type ___________________________

81. For each of the following; predict the products, balance and identify the type of reaction occurring.

_____a. Fe + HCl (assume that the iron ion formed has a +3 charge) type ___________________________

_____b. Ca(OH)2 + HCl type ___________________________

_____c. NaI + Br2 type ___________________________

_____d. Pb(NO3)2 + CuSO4 type ___________________________