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Chem Final Review

Total questions: 99

Worksheet time: 50mins

Name
Class
Date
1.

Which idea of John Dalton is no longer considered part of the modern view of atoms?

a)

Atoms are extremely small

b)

Atoms of the same elements have identical masses

c)

Atoms combine in simple whole number ratios to form compounds

d)

Atoms of different elements can combine in different ratios to form different compounds

2.

energy levels correspond to the

a)

grop number

b)

proton number

c)

period number

3.

each electron will occupy the lowest energy level available and fill in in order

a)

aufbau principle

b)

pauli exclusion principle

c)

hunds rule

4.

two electrons can occupy the same orbital because they have opposite spins

a)

aufbau principle

b)

pauli exclusion principle

c)

hunds rule

5.

single electrons are placed in certain sublevels one at a time with spins in the same direction and then will double up with electrons spinning in opp. directions

a)

aufbau principle

b)

pauli exclusion principle

c)

hunds rule

6.

___ coined the term the atom

a)

Dalton

b)

Democritus

c)

Thomson

d)

Rutherford

7.

proposed that all elements are made up of atoms and that atoms of the same element are alike

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

8.

discovered electrons using the plum pudding model, used the negative cathode ray tube which retracted negative electrons

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

9.

used the gold foil experiment to discover protons and the nucleus

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

10.

determined the energy levels, calculated the # of protons and electrons

a)

Rutherford

b)

Thomson

c)

Bohr

d)

Schrodinger

11.

determined that you cannot precisely locate an electron

a)

Bohr

b)

Chadwick

c)

Thomson

d)

Schrodinger

12.

discovered the neutron and the mass of the neutron

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Chadwick

13.

What is the percent composition of oxygen in KNO3?

a)

0.475%

b)

47.5%

c)

15.8%

d)

23.3%

14.

How many moles of Si are in 50 g of Si?

a)

1404.5 moles

b)

3.01 x 10^25 moles

c)

3.57 moles

d)

1.78 moles

15.

What is the volume, in liters, of 576 g of SO2 gas at STP?

a)

101 L

b)

202 L

c)

216 L

d)

788 L

16.

What is the total number of neon atoms contained in 20.2 grams of Neon gas?

a)

1.01 x 10^24

b)

2.02 x 10^24

c)

3.01 x 10^23

d)

6.02 x 10^23

17.

noble gases have the ___ ionization energy

a)

most

b)

least

18.

Hydrogen and halogens form ___ bonds

a)

single

b)

double

c)

triple

d)

covalent

19.

In order to fill its valence energy level an atom of N is expected to bond with how many atoms of hydrogen?

Hint: Look at the charges

a)

3

b)

1

c)

4

d)

5

20.

2 atoms which have a large difference in electronegativity would form a(n)

a)

ionic bond (cation and anion)

b)

polar covalent bond (two nonmetals)

c)

nonpolar covalent bond

d)

metallic bond

21.

Which of these would not form a covalent bond?

Hint: covalent bonds are made from 2 non-metals

a)

CH4

b)

NH3

c)

Na2O

d)

CO2

22.

What is the difference between dipole-dipole and London dispersion forces?

a)

there is no difference

b)

LDF are usually much weaker than dipole-dipole forces

c)

only LDF are intermolecular

d)

dipole-dipole forces are usually much weaker than LDF

23.

Only extremely polar atoms contain LDF, dipole-dipole, and hydrogen bonding

a)

true

b)

false

24.

only polar covalent atoms have LDF and dipole-dipole forces

a)

true

b)

false

25.

All atoms have LDF

a)

true

b)

false

26.

Most of the compounds in nature, such as H2O, are considered

a)

ionic

b)

covalent

c)

nuclear

d)

metallic

27.

In metals the valence electrons are...

a)

attached to particular positive ions

b)

shared by all of the atoms

c)

immobile

d)

form covalent bonds

28.

Which are exceptions to the sublevel rule (meaning you must take one electron from an s level and move it to the d level)

a)

d9 and d4

b)

d7 and d9

c)

d3 and d4

d)

d9 and d11

29.

the order of the elements in the periodic table is based on

a)

the number of protons in the nucleus

b)

the electron charges

c)

the number of neutrons in the nucleus

d)

atomic mass

30.

Which element has four electrons in its outermost p sublevel at ground state

a)

carbon

b)

chromium

c)

sulfur

d)

promethium

31.

Metallic properties increase down a group

a)

true

b)

false

32.

In relation to the atom, the nucleus has the

a)

most mass and least volume

b)

most mass and most volume

c)

least mass and most volume

d)

least mass and least volume

33.

Atomic # comes from the # of...

a)

neutrons

b)

electrons

c)

protons

34.

Protons and neutrons weigh ___ amu and electrons weigh ___ amu

a)

1, 0

b)

0, 1

c)

1, -1

35.

Element X is located between sodium and potassium on the periodic table. Element X has a

a)

higher atomic # than Potassium

b)

higher atomic mass than Potassium

c)

higher atomic mass than sodium

d)

lower atomic # than sodium

36.

This lab equipment is a(n)....

a)

beaker

b)

balance

c)

graduated cylinder

d)

erlenmeyer flask

37.

___ is measured by how close the calculation is to the true value

a)

precision

b)

accuracy

c)

error

d)

failure percentage

38.

A precise measurement is one that...

a)

contains the correct number of sig figs

b)

is close to the true value

c)

contains 3 sig figs

d)

has measurements close to each other per trial

39.

Sources of error in an experiment could include...

a)

weighing and measuring

b)

amount of oxygen in the air

c)

not giving the subject of the experiment the resources it needs

d)

the subject dies

40.

A process that releases heat is ___ whereas a process that absorbs heat is ___

a)

endothermic, exothermic

b)

exothermic, endothermic

41.

The amount of heat needed to melt one mole of a solid at a constant temperature is called _______

a)

heat of reaction

b)

enthalpy

c)

heat of vaporization

d)

heat of fusion

42.

The amount of heat needed to evaporate one mole of a solid at a constant temperature is called _______

a)

heat of reaction

b)

enthalpy

c)

heat of vaporization

d)

heat of fusion

43.

On what principle does calorimetry depend?

a)

law of multiple proportions

b)

Hess's Law

c)

Law of Enthalpy

d)

Law of Conservation of Energy

44.

How do you determine how much excess reactant is left over?

a)

1. Find which reactant is the limiting by converting it to the product (whichever produces less is the limiting)

2. convert the limiting to grams of the excess

3. subtract what you calculated from what you were given

b)

1. Convert the product to each reactant

2. subtract the product from the limiting

3. subtract the calculated amount of product from the given amount of reactant

c)

1. determine the excess by converting it to the product

2. convert the excess to grams of the limiting

3. subtract what you calculate from what you're given

d)

all of these methods work

45.

When 200 g of sulfur reacts with 100.3 g of chlorine to produce disulfur dichloride, how much excess reactant is left over?

                   2S + Cl2   --> S2Cl2

a)

0.773 g S

b)

20.26 g S

c)

40.5 g S

d)

109.3 g S

46.

How many grams of O2 are required to produce 358.5 grams of ZnO?

2Zn + O2 --> 2ZnO

a)

29.1 g

b)

70.5 g

c)

1302 g

d)

14.5 g

47.

How many moles of Al would be produced from 20 moles of Al2O3?

2Al2O3 --> 4Al + 3O2

a)

4 moles Al

b)

40 moles Al

c)

10 moles Al

d)

20 moles Al

48.

According to this chemical reaction, which is the number of grams of Fe produced from 14 moles of H2?

Fe3O4 (cr) + 4 H2 (g) --> 3 Fe (cr) + 4 H2O (l)

a)

4862.1 g Fe

b)

2431.3 g Fe

c)

587.2 g Fe

d)

22.1 g Fe

49.

You go camping and roast marshmallows over a campfire.  What happens to the volume of the air bubbles inside the marshmallows?

a)

increase

b)

decrease

50.

The pressure in an automobile tire is 1.88 atm at 25.0°C. What will be the pressure if the temperature warms up to 37.0°C?

a)

1.27 atm

b)

1.96 atm

c)

3.45 atm

d)

2.78 atm

51.

The initial volume of a gas at a pressure of 3.2 atm is 2.9 L. What will the volume be if the pressure is increased to 4.0 atm?

a)

4.41 atm

b)

1.6 atm

c)

2.32 atm

d)

2.5 atm

52.

Calculate the number of moles in 150 g of Mg.

a)

3646.5 mol

b)

3647 g

c)

6.17 mol

d)

6.17 g

53.

Calculate the number of grams in 15 moles of O2

a)

239.985 g

b)

239.985 g

c)

479.97 mol

d)

479.97 g

54.

Calculate the molar mass for the following compound: 

Magnesium Hydroxide 

a)

41.32 g/mol

b)

58.32 g/mol

c)

40.31 g/mol

d)

82.64 g/mol

55.

Avogadro's number is equal to 6.02x1023

a)

true

b)

false

56.

In the following compound how many hydrogen atoms are there?

2(NH4)2S

a)

2

b)

4

c)

8

d)

16

57.

What type of reaction is the following?

Fe + Cu(NO3)2 ---> Fe(NO3)2 + Cu

a)

single displacement

b)

double displacement

c)

decomposition

d)

synthesis

58.

_____Cl2+ _____NaBr → _____NaCl + _____Br2

Choose the appropriate coefficient for NaBr

a)

3

b)

2

c)

4

d)

1

59.

Name FeSO4

a)

Iron (I) sodium tetroxide

b)

Iron (I) sulfate

c)

Iron (II) sodium oxide

d)

Iron (II) sulfate

60.

Choose the formula for:

Dibromine tetrahydride

a)

B2H4

b)

Br2H4

c)

Br3H4

61.

The type of bond that forms between Mg and Cl is ___

a)

ionic

b)

covalent

c)

polar

d)

nonpolar

62.

Choose the formula for:

Cobalt (II) Bromide

a)

CoBr2

b)

Co2Br

c)

Cl2Br

63.

Name the following compound:

NBr4

a)

nitrogen tetrabromide

b)

nitrogen bromide

c)

nitrogen (II) bromide

d)

nitrogen tetrabromide

64.

Name the following compound:

Ca(ClO)2

a)

calcium dichlorine dioxide

b)

calcium hypochlorite

c)

calcium chloride oxide

d)

calcium carbonate

65.

What is the formula for:

Sodium Carbonate

a)

NaCO

b)

NaCO3

c)

Na2CO

d)

Na2CO3

66.

Carbon bonds with Bromine. What bond is formed?

a)

Covalent because they are both metals

b)

Covalent because they are both nonmetals

c)

Ionic because carbon is a metal and bromine is a nonmetal

d)

ionic because they are both nonmetals

67.

electronegativity ___ down and to the left

a)

decreases

b)

increases

68.

ionization energy ___ up and to the right

a)

increases

b)

decreases

69.

Atomic radius ___ from left to right across a period

a)

increases

b)

decreases

70.

elements in the same group have the same number of ___

a)

electrons

b)

neutrons

c)

valence electrons

d)

protons

71.

anions become negatively charged ions by gaining electrons

a)

true

b)

false

72.

cations (metals) become positively charged ions by losing electrons

a)

true

b)

false

73.

When Sodium gives up an electron it becomes a positively charged ion

a)

true

b)

false

74.

the f sublevel has ___ orbitals and ___ electrons

a)

one, two

b)

three, six

c)

five, ten

d)

seven, fourteen

75.

the d sublevel has ___ orbitals and ___ electrons

a)

one, two

b)

three, six

c)

five, ten

d)

seven, fourteen

76.

the p sublevel has ___ orbitals and ___ electrons

a)

one, two

b)

three, six

c)

five, ten

d)

seven, fourteen

77.

The s sublevel has ___ orbital and can hold ___ electrons

a)

one, two

b)

three, six

c)

five, ten

d)

seven, fourteen

78.

The second energy level can hold up to ___ electrons

a)

2

b)

6

c)

8

d)

18

79.

The first energy level can hold up to ___ electrons

a)

2

b)

6

c)

8

d)

18

80.

Identify the number of protons, neutrons, and electrons in phosphorus.

a)

31 protons, 15 neutrons, and 31 electrons

b)

15 protons, 16 neutrons, and 15 electrons

c)

15 protons, 14 neutrons, and 14 electrons

81.

Which best describes the current atomic theory?

a)

Atoms consist if electrons circling in definite orbits around a positive nucleus

b)

Atoms are composed of electrons in a cloud around a positive nucleus

c)

Atoms can easily be split at which time they become radioactive

82.

Scientific hypotheses are most often tested by the process of...

a)

communicating

b)

inferring

c)

experimenting

d)

analyzing data

83.

In order to find the volume of a liquid accurately use a(n) ___ while to find the mass of an object use a(n)___.

a)

balance; graduated cylinder

b)

Erlenmeyer flask; balance

c)

graduated cylinder; balance

d)

beaker; graduated cylinder

84.

A scientist is conducting an experiment in which she measures the density of water. What might result in inconclusive results?

a)

The volume of the water was slightly different each time

b)

the balance was not zeroed each time

c)

the mass of the water was different each time

d)

all of the above

85.

Element X is located between Na and K on the periodic table. Which statement is correct about element X?

a)

It has a higher atomic # then K

b)

It has a higher atomic mass than K

c)

It has a higher atomic mass than Na

d)

It has a lower atomic # than Na

86.

In relation to the atom, the nucleus has...

a)

most mass and least volume

b)

most mass and most volume

c)

least mass and most volume

d)

least mass and least volume

87.

Which of the following would be considered isotopes of Beryllium?

i. Element A: atomic number 4, mass 9

ii. Element B: atomic number 4, mass 10

iii. Element C: atomic number 5, mass number 9

iv. Element D: atomic number 3, mass 9

a)

element A and B

b)

element A only

c)

element A, C, and D

d)

element C only

88.

The order of elements on the periodic table is based on...

a)

the number of protons in the nucleus

b)

the electric charge of the nucleus

c)

the number of neutrons in the nucleus

d)

atomic mass

89.

Using the periodic table, identify which of the following Group 15 elements has the most metallic properties?

a)

Bi

b)

Sb

c)

P

d)

N

90.

An element has an electron configuration of 1s2 2s2 2p6 3s2 3p1

How many electrons can this element donate when it forms an ionic bond?

a)

13

b)

3

c)

2

d)

1

91.

Which of the following electron configurations describes a halogen?

a)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6

b)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p5

c)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4

d)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3

92.

The idea that two electrons can occupy the same orbital because they have opposite spins is part of the...

a)

Pauli Exclusion Principle

b)

Aufbau Principle

c)

Hund's Rule

d)

The Electron Orbital Rule

93.

The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge is...

a)

J.J. Thompson

b)

Lord Kelvin

c)

Ernest Rutherford

d)

Robert Millikan

94.

Which set of elements are alkali metals?

a)

helium, neon, and argon

b)

Lithium, sodium, and potassium

c)

beryllium, magnesium, and calcium

d)

boron, aluminum, and gallium

95.

using a periodic table, how many protons, electrons, and then neutrons are in an atom of potassium

a)

39, 19, 19

b)

19, 19, 20

c)

19, 20, 19

d)

19, 19, 19

96.

Which set of elements has 1 electron for bonding

a)

hydrogen and helium

b)

lithium and fluorine

c)

helium and neon

d)

lithium and sodium

97.

All atoms contain of the same element contain the same number of ___

a)

neutrons

b)

electrons

c)

valence electrons

d)

protons

98.

Protons have a ___ charge

a)

neutral

b)

negative

c)

positive

99.

the overall charge of an atom is ___

a)

negative

b)

positive

c)

neutral

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