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Accelerated Chemistry > Final Review Packet > Flashcards

Final Review Packet Flashcards

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1
Q

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

A
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2
Q

Given the following thermochemical equations

H2(g) + 1⁄2O2(g) —> H2O(ℓ)

ΔH° = -285.8 kJ

A
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3
Q
  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
A
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4
Q

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

A
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5
Q

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)

A
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6
Q

How many seconds in 150 weeks?

A
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7
Q

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

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

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8
Q

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

A
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9
Q

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

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

A
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10
Q

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

d. Lithium + oxygen →

A
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11
Q

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

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

A
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12
Q

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

Provide an example using sulfur, sulfate and sulfite.

A
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13
Q

Given the following equation:

2 C + 2 H2O → CH4 + CO2

ΔHrxn= 15 kJ

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

A
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14
Q

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

A
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15
Q

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

A
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16
Q

Where are metals found on the periodic table?

Metalloids?

Nonmetals?

Give an example of each.

A
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17
Q

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

A
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18
Q

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

A
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19
Q

Given the following thermochemical equations

C(s) + O2(g) —> CO2(g)

ΔH° = -393.5 kJ

A
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20
Q

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

A
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21
Q

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)

A
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22
Q

What makes the noble gases unique?

A
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23
Q

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

aluminum reacts with fluorine gas

A
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24
Q

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

A
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25
Q

How many atoms are there in 502 g of Al?

A
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26
Q

What are the differences between physical changes and chemical changes?

A
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27
Q

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?

A
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28
Q

Write orbital notation for each of the following (ignore core electrons):

a. P
b. Mn
c. Sn

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29
Q

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

A
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30
Q

Using the following reaction:

C5H12 + 8 O2 → 5 CO2 + 6 H2O

ΔHc = -3509 kJ/mol

Calculate ΔHc if 234.6 g of pentane reacts completely in the reaction shown above

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31
Q

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

A
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32
Q

Explain the following.

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

A
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33
Q

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

A
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34
Q

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

A
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35
Q

Given the following equation:

2 C + 2 H2O → CH4 + CO2

ΔHrxn= 15 kJ

b. What will be the ΔH if 1250g of carbon react with excess water?

A
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36
Q

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

A
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37
Q

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 = ???

A
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38
Q

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?

A
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39
Q

Calculate the enthalpy for this reaction:
2C(s) + H2(g) —> C2H2(g)

ΔH° = ??? kJ

A
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40
Q

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

A
41
Q

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?

A
42
Q

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

c. Calcium nitride →

A
43
Q

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

A
44
Q

On the periodic table, the horizontal rows are called: __________ .

The vertical columns are called _________ or __________ .

Which of these contains elements with similar properties?

A
45
Q

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

f. NaF + AlPO4 →

A
46
Q

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 →

A
47
Q

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?

A
48
Q

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

A
49
Q

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

A
50
Q

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

A
51
Q

Why don’t zinc and silver need Roman Numerals?

Provide an example compound for each

A
52
Q

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?

A
53
Q

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?

A
54
Q

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

A
55
Q

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

sulfuric acid reacts with sodium hydroxide

A
56
Q

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

A
57
Q

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

A
58
Q

Write the following numbers in scientific notation:

a. 3500000
b. 0.0004
c. 444000000000000

A
59
Q

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

A
60
Q

An aluminum brick with a mass of 2135g is heated to a temperature of 150oC and dropped into a bucket containing 5.50 kg of water initially at a temperature of 17.0oC.

Determine the final temperature of the mixture.

(cAl = .904 J/goC)

A
61
Q

For red light with a wavelength of 685nm,

a. Determine the frequency of light.
b. Calculate the energy per photon of the light

A
62
Q

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

A
63
Q

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

a. C5H10 + O2 →

A
64
Q

Answer the following questions about naming compounds (nomenclature).

a. Why are Roman Numerals used? Which compounds need Roman Numerals following the name?

A
65
Q

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

A
66
Q

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

A
67
Q

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

A
68
Q

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

A
69
Q

What is the percent composition of hydrogen in acetic acid?

A
70
Q

Predict the products, balance the molecular equation and determine whether the products are soluble or insoluble of the following (use the solubility chart).

d. Iron (III) chloride + calcium nitrate

A
71
Q

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?
A
72
Q

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?

A
73
Q

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

e. Zinc + sodium chloride →

A
74
Q

Given the following equation:

2 C + 2 H2O → CH4 + CO2

ΔHrxn= 15 kJ

a. Is the reaction above exothermic or endothermic? Explain briefly.

A
75
Q

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?

A
76
Q

Write the full electron configuration for each of the following:

a. Mg2+
b. S2-
c. C* (an excited state of carbon)

A
77
Q

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

A
78
Q

Which seven elements naturally occur as diatomic molecules?

A
79
Q

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

A
80
Q

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

A
81
Q

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

A
82
Q

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

b. Aluminum + nickel (II) sulfate →

A
83
Q

Given the following thermochemical equations:
C2H2(g) + 5⁄2O2(g) —> 2CO2(g) + H2O(ℓ)

ΔH° = -1299.5 kJ

A
84
Q

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

A
85
Q

What are two types of separation techniques?

How do they work?

What type of mixture do they separate?

A
86
Q

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?

A
87
Q

Name the following compounds:

a. K2SO3
b. FeS
c. H2SO3
d. CaO

e. HF
f. NF2

g. PCl5
h. Na2Cr2O7
i. MgCO3

A
88
Q

Sketch an “s” and “p”orbital.

A
89
Q

Write the noble gas configuration for each of the following:

a. Al
b. As
c. Os
d. Cs

A
90
Q

Write the full electron configuration for the following:

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

A
91
Q

Explain how to name covalent compounds. Provide an example.

A
92
Q

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?

A
93
Q

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

A
94
Q

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

A
95
Q

What is the maximum number of electrons that can occupy

a. The n=3 energy level ___
b. The 4d sublevel___
c. A 2px orbital___
d. The 5f sublevel___
e. The 7s sublevel___

A
96
Q

Balance the following equations:

a. ___ Al + ___ NiSO4 → ___ Ni + ___ Al2(SO4)3

A
97
Q

Balance the following equations:

b. ___Cu2S + ___ O2 → ____ Cu2O + ___ SO2

A
98
Q

Balance the following equations:

c. ___ C3H8 + ___ O2 → ___ H2O + ___ CO2

A

Accelerated Chemistry (9 decks)

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