Final Review Packet

Question 1

How many sig figs in the following numbers?

a. 308 apples
b. 0.0008 cm
c. 200 seconds
d. 40. milliliters
e. 607.03 kilograms
f. 77.0 quarts

Question 2

Given the following thermochemical equations

H₂(g) + ^1⁄₂O₂(g) —> H₂O(ℓ)

ΔH° = -285.8 kJ

Question 3

1. An electron in hydrogen drops from the n=6 to n=2 energy level and releases a photon of violet light.
2. If an electron dropped from the n=7 to n=2 energy level, what type of radiation would you expect to be released?
3. Explain briefly

Question 4

Find the empirical formula for a compound with the following percent composition: 36.1% Ca, 63.9% Cl

Question 5

Do the following math problems, and be sure your answers have the correct number of sig figs.

a. 3.4 g + 61 g
b. 493 mL + 5.0 mL
c. 390 g / 6.999 cm³
d. 3.74 L – 171.11 L
e. (966 m)(420 m)

Question 6

How many seconds in 150 weeks?

Question 7

Determine which of the following is a physical change or a chemical change:

a. burning ____
b. melting ____
c. dissolving ____
d. digesting ____
e. changes color _____

Question 8

What are the two types of mixtures? Give an example of each.

Question 9

Determine which of the following is a physical property, or a chemical property:

a. length _____
b. density _____
c. temperature ____
d. flammability ____
e. reactivity _____

Question 10

Predict products, balance the equation and name the type of reaction for the following:

d. Lithium + oxygen →

Question 11

For a-d below, circle the valence electrons in each configuration.

a. Br
b. Zn
c. O
d. Y

Question 12

List the three rules to name acids. (Binary, Polyatomic ions (-ate), Polyatomic ions (-ite)).

Provide an example using sulfur, sulfate and sulfite.

Question 13

Given the following equation:

2 C + 2 H₂O → CH₄ + CO₂

ΔH_rxn= 15 kJ

c. If I produce 290g CO₂ from 480g H₂O, what is my % yield?

Question 14

What is the mass of 4.55 x 10²⁴ molecules of nitrous acid?

Question 15

How can you tell the difference between an ionic compound and a covalent compound?

Question 16

Where are metals found on the periodic table?

Metalloids?

Nonmetals?

Give an example of each.

Question 17

Describe the difference between a sodium atom in its ground state versus a sodium atom in an excited state.

Question 18

Write the following numbers in standard notation.

a. 9.200000 x 10^-4
b. 3.6 x 10³
c. 8 x 10⁵
d. 4.11 x 10^-3

Question 19

Given the following thermochemical equations

C(s) + O₂(g) —> CO₂(g)

ΔH° = -393.5 kJ

Question 20

For each of the following:
a) predict the products and balance the equation

b) write the complete ionic equation
c) write the net ionic equation
d) list any precipitates
e) list any spectator ions

a. mercury (II) chloride + potassium sulfide

Question 21

In each of the following change the number of significant figures indicated in parenthesis:

a. 0.0002356 (3 sig figs)
b. 22.0500689 (4 sig fgs)
c. 1.0000 (2 sig figs)

Question 22

What makes the noble gases unique?

Question 23

Predict the products and write a balanced equation for the following reaction:

aluminum reacts with fluorine gas

Question 24

What four types of evidence are signs a chemical change has occurred?

Question 25

How many atoms are there in 502 g of Al?

Question 26

What are the differences between physical changes and chemical changes?

Question 27

Given the following equation: iron (III) hydroxide + sulfuric acid → iron (III) sulfate + water If you have 427g of iron III hydroxide, and 638g of sulfuric acid… c. How many molecules of water are produced?

Question 28

Write orbital notation for each of the following (ignore core electrons): a. P b. Mn c. Sn

Question 29

Give an example of a compound that has both ionic and covalent bonds holding atoms together.

Question 30

Using the following reaction: C₅H₁₂ + 8 O₂ → 5 CO₂ + 6 H₂O ΔHc = -3509 kJ/mol Calculate ΔH_c if 234.6 g of pentane reacts completely in the reaction shown above

Question 31

List the components to Daltons Atomic Theory, and circle the 2 that were later proven incorrect

Question 32

Explain the following. a. Aufbau Principle: b. Hund’s Rule: c. Pauli Exclusion Principle

Question 33

What are the parts of an atom, their charges and where they are located?

Question 34

What is the symbol, atomic number, avg. atomic mass, and the number of electrons, protons and neutrons of: a. Sodium b. Sulfur c. Neon d. Lead e. Copper f. Iron g. Silicon

Question 35

Given the following equation: 2 C + 2 H₂O → CH₄ + CO₂ ΔH_rxn= 15 kJ b. What will be the ΔH if 1250g of carbon react with excess water?

Question 36

What are two types of pure substances? Give an example of each.

Question 37

Given the following information: 2NO(g) + O2(g) ---\> 2NO2(g) ΔH = -116 kJ 2N₂(g) + 5O₂(g) + 2H₂O(ℓ) ---\> 4HNO₃(aq) ΔH = -256 kJ N2(g) + O2(g) ---\> 2NO(g) ΔH = +183 kJ Calculate the enthalpy change for the reaction below: 3NO2(g) + H2O(ℓ) ---\> 2HNO3(aq) + NO(g) ΔH = ???

Question 38

Using the following reaction: C₅H₁₂ + 8 O₂ → 5 CO₂ + 6 H₂O ΔHc = -3509 kJ/mol How many moles of C₅H₁₂ are required to make 6.16 mole of water?

Question 39

Calculate the enthalpy for this reaction: 2C(s) + H₂₍g) ---\> C₂H₂(g) ΔH° = ??? kJ

Question 40

For each of the following: a) predict the products and balance the equation b) write the complete ionic equation c) write the net ionic equation d) list any precipitates e) list any spectator ions **c. copper (II) hydroxide + hydrobromic acid**

Question 41

Given the following equation: iron (III) hydroxide + sulfuric acid → iron (III) sulfate + water If you have 427g of iron III hydroxide, and 638g of sulfuric acid… b. How many grams of iron (III) sulfate are produced?

Question 42

Predict products, balance the equation and name the type of reaction for the following: c. Calcium nitride →

Question 43

Determine the average atomic mass of strontium based on the following data: Isotope - ⁸⁴Sr, ⁸⁶Sr, ⁸⁷Sr, ⁸⁸Sr Atomic mass of isotope (amu) - 83.913, 85.909, 86.909, 87.906 Percent abundance (%) - 0.56 , 9.86, 7.00 , 82.58

Question 44

On the periodic table, the horizontal rows are called: __________ . The vertical columns are called _________ or __________ . Which of these contains elements with similar properties?

Question 45

Predict products, balance the equation and name the type of reaction for the following: f. NaF + AlPO₄ →

Question 46

For each of the following: a) predict the products and balance the equation b) write the complete ionic equation c) write the net ionic equation d) list any precipitates e) list any spectator ions **b. Na₂CO₃ + CaCl₂ →**

Question 47

Given the following equation: iron (III) hydroxide + sulfuric acid → iron (III) sulfate + water If you have 427g of iron III hydroxide, and 638g of sulfuric acid… a. What is the limiting reagent? What is the excess reagent?

Question 48

Calculate the wavelength of radio waves with a frequency of 98.7 MHz.

Question 49

If a compound has an empirical formula of C₂H₃ , and a molar mass of 216.5 g/mol, what is the molecular formula?

Question 50

How many moles of Br are in 33.04 g of CaBr₂?

Question 51

Why don’t zinc and silver need Roman Numerals? Provide an example compound for each

Question 52

Using the following reaction: C₅H₁₂ + 8 O₂ → 5 CO₂ + 6 H₂O ΔHc = -3509 kJ/mol How many grams of C₅H₁₂ are needed to make 9.70 moles of carbon dioxide?

Question 53

Lithium has two isotopes, lithium-6 and lithium-7. (Assume their masses are 6.00amu and 7.00amu). If the average atomic mass of lithium is 6.941amu, what percent of each isotope occurs naturally?

Question 54

Predict the products, balance the molecular equation and determine whether the products are soluble or insoluble of the following (use the solubility chart). **b. Sodium carbonate + barium chloride**

Question 55

Predict the products and write a balanced equation for the following reaction: sulfuric acid reacts with sodium hydroxide

Question 56

Write the correct formula for the following compounds: a. barium hydroxide b. acetic acid c. calcium chloride d. zinc nitrate e. manganese (II) phosphate f. hydrosulfuric acid g. copper (IV) sulfite h. heptasilicon tetraoxide i. dinitrogen hexafluoride

Question 57

Predict the products, balance the molecular equation and determine whether the products are soluble or insoluble of the following (use the solubility chart). **a. Barium chloride + silver nitrate**

Question 58

Write the following numbers in scientific notation: a. 3500000 b. 0.0004 c. 444000000000000

Question 59

If the density of a metal is 3.60 g/cm³, what is the volume of a 17.0 g sample?

Question 60

An aluminum brick with a mass of 2135g is heated to a temperature of 150^oC and dropped into a bucket containing 5.50 kg of water initially at a temperature of 17.0^oC. Determine the final temperature of the mixture. (c_Al = .904 J/g^oC)

Question 61

For red light with a wavelength of 685nm, a. Determine the frequency of light. b. Calculate the energy per photon of the light

Question 62

When do you need to use “hydro” in naming acids? Provide an example.

Question 63

Predict products, balance the equation and name the type of reaction for the following: a. C₅H₁₀ + O₂ →

Question 64

Answer the following questions about naming compounds (nomenclature). a. Why are Roman Numerals used? Which compounds need Roman Numerals following the name?

Question 65

Do lead and tin need Roman Numerals? Provide an example compound for each.

Question 66

What is the name and complete chemical formula of the hydrate of sodium carbonate based on the following lab analysis: Initial mass of hydrate: 7.441 g sodium carbonate hydrate Mass after heating to dryness: 2.761 g anhydrous sodium carbonate

Question 67

How many formula units of barium hydroxide are there in 1.81 moles of barium hydroxide?

Question 68

What are the important differences between the Bohr model of the atom and the Quantum Mechanical model?

Question 69

What is the percent composition of hydrogen in acetic acid?

Question 70

Predict the products, balance the molecular equation and determine whether the products are soluble or insoluble of the following (use the solubility chart). ## Footnote **d. Iron (III) chloride + calcium nitrate**

Question 71

Given the following equation: Zinc + hydrochloric acid → (predict the products and balance the equation) * If you start with 164g of Zn and 219g of HCl…* a. What is the limiting reagent? What is the excess reagent?

Question 72

Using the following reaction: C₅H₁₂ + 8 O₂ → 5 CO₂ + 6 H₂O ΔHc = -3509 kJ/mol How many moles of water are produced from 3.70 moles of oxygen?

Question 73

Predict products, balance the equation and name the type of reaction for the following: e. Zinc + sodium chloride →

Question 74

Given the following equation: 2 C + 2 H₂O → CH₄ + CO₂ ΔH_rxn= 15 kJ a. Is the reaction above exothermic or endothermic? Explain briefly.

Question 75

Given the following equation: Zinc + hydrochloric acid → (predict the products and balance the equation) If you start with 164g of Zn and 219g of HCl… b. How many grams of ZnCl₂ will be produced?

Question 76

Write the full electron configuration for each of the following: a. Mg²⁺ b. S^2- c. C\* (an excited state of carbon)

Question 77

All atoms of the same element have the same number of _________ and __ \_\_\_\_\_\_\_\_\_, but may have different numbers of __________ .

Question 78

Which seven elements naturally occur as diatomic molecules?

Question 79

What are the names of the following groups: a. group 1A b. group 2A c. group 3-12 d. group 7A e. group 8A f. elements with atomic #’s 57-70 & 89-102

Question 80

What is the mass of 1.62 x 10²⁴ atoms of sodium?

Question 81

If a compound has an empirical formula of NO₂, and a mass of 92 grams, what is the molecular formula?

Question 82

Predict products, balance the equation and name the type of reaction for the following: b. Aluminum + nickel (II) sulfate →

Question 83

Given the following thermochemical equations: C₂H₂(g) + ^5⁄₂O₂(g) ---\> 2CO₂(g) + H₂O(ℓ) ΔH° = -1299.5 kJ

Question 84

Predict the products, balance the molecular equation and determine whether the products are soluble or insoluble of the following (use the solubility chart). **c. Lead (II) nitrate + sodium carbonate**

Question 85

What are two types of separation techniques? How do they work? What type of mixture do they separate?

Question 86

A compound has a percent composition is: 58.8 % C, 9.9 % H, and 31.3 % O. If it’s molecular mass is 306 g/mole, what is the molecular formula?

Question 87

Name the following compounds: a. K₂SO₃ b. FeS c. H₂SO₃ d. CaO e. HF f. NF₂ g. PCl₅ h. Na₂Cr₂O₇ i. MgCO₃

Question 88

Sketch an “s” and “p”orbital.

Question 89

Write the noble gas configuration for each of the following: a. Al b. As c. Os d. Cs

Question 90

Write the full electron configuration for the following: a. Br b. Zn c. O d. Y

Question 91

Explain how to name covalent compounds. Provide an example.

Question 92

Using the following reaction: C₅H₁₂ + 8 O₂ → 5 CO₂ + 6 H₂O ΔHc = -3509 kJ/mol How many grams of carbon dioxide form at the same time as 4.29 grams of water?

Question 93

For the following types of electromagnetic radiation, rank each from LOWEST energy to HIGHEST energy. Yellow light UV Microwaves Blue light Radio Waves Red Light Gamma IR

Question 94

What is the percent composition of each element in aluminum hydroxide?

Question 95

What is the maximum number of electrons that can occupy a. The n=3 energy level \_\_\_ b. The 4d sublevel\_\_\_ c. A 2p_x orbital\_\_\_ d. The 5f sublevel\_\_\_ e. The 7s sublevel\_\_\_

Question 96

Balance the following equations: a. ___ Al + ___ NiSO₄ → ___ Ni + ___ Al₂(SO₄)₃

Question 97

Balance the following equations: b. \_\_\_Cu₂S + ___ O₂ → ____ Cu₂O + ___ SO₂

Question 98

Balance the following equations: c. ___ C₃H₈ + ___ O₂ → ___ H₂O + ___ CO₂