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TSNF Final

Total questions: 114

Worksheet time: 53mins

Name
Class
Date
1.
What is the the shape of this molecule according to VSPER theory?
a)
Linear
b)
Tetrahedral
c)
Trigonal Planar
d)
Trigonal pyramidal
2.

What compound could this be?

a)

CO2

b)

NH3

c)

H2S

d)

CH4

3.

Draw the Lewis Dot structure for PCl5 and determine the predicted molecular geometry

a)

octahedral

b)

trigonal pyramidal

c)

seesaw

d)

trigonal bipyramidal

4.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
5.
How many sigma and pi bonds does this have?
a)
1 sigma and 1 pi
b)
2 sigma and 1 pi
c)
1 sigma and 2 pi
d)
2 sigma and 2 pi
6.
How many sigma and pi bonds does this have? 
a)
3 sigma and 2 pi
b)
5 sigma and 5 pi
c)
5 sigma and 0 pi
d)
0 sigma and 5 pi
7.
Carbon atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
8.

Filtering separates mixtures based on differences in what property?

a)

Chemical

b)

Solubility

c)

Particle size

d)

Density

9.

What is the equation for calculating the density of a substance?

a)

D=m/v

b)

m=D/v

c)

D=v*m

d)

D=v/m

10.

When an electron is in a lower energy level, it is ________________ away from the nucleus

a)

Closer

b)

Farther

11.

When reading a PES (Photoelectric Spectroscopy) graph, what does the height of a peak represent?

a)

The number of electrons

b)

The number of protons

c)

The mass or the isotope

d)

The amount of energy the electron has

12.

Isotopes of an element have the same number of __________, but different number of __________.

a)

protons, neutrons

b)

neutrons, protons

c)

protons, electrons

d)

electrons, protons

13.

When reading a PES (Photoelectron Spectroscopy) graph, a larger binding energy means that the electrons are _________________ the nucleus?

a)

Closer to

b)

Farther from

14.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

15.

What type of change conserves mass?

a)

none

b)

chemical

c)

physical

d)

chemical and physical

16.

When an electron is in a higher energy level, it has ___________ Coulombic attraction to the nucleus

a)

More

b)

Less

17.

What is the measurement of the burette? (in mL)

a)

6.6mL

b)

6.64mL

c)

7.36mL

d)

7.3mL

18.

Which orbital comes after 4s?

a)

3d

b)

5s

c)

4p

d)

4d

19.

Are cations larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

20.

Which piece of glassware is the most precise

a)

beaker

b)

graduated cylinder

c)

burette

d)

test tube

21.

Moving across a row (L to R) on the periodic table, Zeff _________________

a)

Increases

b)

Decreases

c)

Stays the same

22.

What type of change separates a compound into elements?

a)

physical

b)

chemical

c)

chemical and physical

23.

Why do atoms get smaller moving across a period (L to R) on the periodic table?

a)

More protons (q) to attract the electrons

b)

Fewer protons (q) to attract the electrons

c)

More energy shells (r) so it can't attract the electrons

d)

Fewer energy shells (r) so it attracts the electrons closer

24.

Why are anions larger than their neutral atoms?

a)

More shielding that repels the other electrons

b)

Fewer protons to attract electrons

c)

More electrons to attract protons

d)

More Zeff to attract electrons

25.

Which piece of glassware is the least precise?

a)

graduated cylinder

b)

beaker

c)

burette

26.

When an electron is in a lower energy level, it has a ________________ 1st ionization energy

a)

Higher

b)

Lower

c)

Same

27.

What is the total # of covalent bonds carbon has to make when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

28.

Which electrons are removed first when making a cation?

a)

s

b)

p

c)

d

d)

f

29.

What do mass spectroscopy graphs measure?

a)

Mass of isotopes

b)

Mass of protons

c)

Energy of electrons

d)

Number of electrons

30.

What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

31.

When reading a PES graph, a larger binding energy means that the electrons are ____________ from the nucleus?

a)

closer

b)

farther

c)

the same distance

32.

Which orbital comes after 4p?

a)

5s

b)

4s

c)

3d

d)

4p

33.

What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

109.5

34.

Fill in the blanks germanium is a ________________, hydrogen is a _________________ and uranium is a ________________

a)

metal, non-metal, metalloid

b)

metalloid, non-metal, metal

c)

non-metal, metal, metalloid

35.

Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

36.

What is the bond angle in NH3

a)

120

b)

109.5

c)

180

d)

90

37.

List the 3 Intermolecular forces from weakest to strongest

a)

hydrogen bonding, london dispersion, dipole dipole

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole, hydrogen bonding

d)

dipole dipole, hydrogen bonding, london dispersion

38.

List ALL the Intermolecular forces that exist in PCl3

a)

hydrogen bonding, london dispersion

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole

d)

london dispersion

39.

Are anions larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

40.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

41.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

42.

Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

43.

P and V are ___________________ related?

a)

inversely

b)

directly

44.

The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

45.

Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

46.

Real gases behave most like an ideal gas at what conditions of temperature and pressure?

a)

High T, Low P

b)

High P, Low T

c)

High V, Low T

47.

When an electron is in a lower energy level, it has a ___________ 1st ionization energy

a)

Higher

b)

Lower

48.

What is the hybrid orbital used in CH4?

a)

sp3

b)

sp

c)

sp2

49.

What is the hybrid orbital used in CO2

a)

sp3

b)

sp

c)

sp2

50.

Count the number of sigma and pi bonds in this molecule:

a)

13 sigma, 1 pi

b)

14 sigma, 2 pi

c)

1 sigma, 14 pi

d)

2 sigma, 13 pi

51.

Why are asymmetrical molecules polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

52.

What is the bond angle in SO2

a)

120

b)

90

c)

180

d)

109.5

53.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

54.

When a molecular solid melts or boils, which bonds break?

a)

Intermolecular

b)

Intramolecular

55.

What type of alloy is made when the radii of the atoms are similar in size?

a)

interstitial

b)

substitutional

56.

This is a representation of a hydrogen bond.

a)

True

b)

False

57.

This is a representation of a hydrogen bond.

a)

True

b)

False

58.

Which atom has the negative dipole in this molecule?

a)

Hydrogen

b)

Fluorine

c)

Neither

59.

In this molecule, Carbon has a formal charge of ____ and Nitrogen has a formal charge of _____.

a)

0, 0

b)

1, 0

c)

0, -1

d)

-1, 0

60.

What is the formula for calculating % yield?

a)

actual/theoretical *100

b)

theoretical/actual *100

61.

What is a limiting reactant?

a)

The reactant that runs out first

b)

The reactant that has the lowest mass

c)

The reactant with the smallest coefficient

d)

The reactant with the lowest molar mass

62.

Combustion reactions produce what two substances?

a)

Water Vapor and Carbon Dioxide

b)

Carbon Dioxide and Oxygen

c)

Oxygen and Water Vapor

63.

As the electronegativity difference between 2 atoms increases, the polarity of the bond ____________________

a)

increases

b)

decreases

64.

What type of bond forms between hydrogen and chlorine?

a)

polar covalent

b)

non-polar covalent

c)

ionic

d)

hydrogen bond

65.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

66.

dRT/P equals what quantity?

a)

Molar mass

b)

Volume

c)

Vapor pressure

d)

Mass

67.

What is the unit for the rate constant (k) for 1st order reactions?

a)

s-1

b)

M/s

c)

M-1s-1

68.

What is the oxidation number of P in PO43-?

a)

0

b)

4

c)

5

d)

-2

69.

What formula do we use for dilution calculations?

a)

M1V1=M2V2

b)

D=m/V

c)

V1=M2

d)

Total Volume/Partial Volume

70.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

71.

What order is this graph?

a)

Zero

b)

First

c)

Second

d)

Third

72.

What is the oxidation number of N in NO21-?

a)

0

b)

-1

c)

2

d)

3

73.

The lewis structure on the ___________ is better because ________________

a)

left, formal charges are zero

b)

left, the formal charges equal -1

c)

right, formal charges are zero

d)

right, the formal charges equal -1

74.

If you quadruple the concentration and the rate quadruples, what order is this reaction?

a)

zero

b)

first

c)

second

75.

What is the electron configuration of Phosphorus?

a)

1s2 2s2 2p6 3s2 3p3

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 4p3

d)

1s2 2s2 2p6 3s2 3p5

76.

Which step of a reaction mechanism determines the rate?

a)

the slow step

b)

the fast step

c)

the first step

d)

the second step

77.

What order is the half life of Carbon14?

a)

Zero

b)

First

c)

Second

78.

1.What type of reaction is this?

3O2 + 2FeCl3 --> 2Fe2O3 + 3Cl2

a)

Single Displacement

b)

Decomposition

c)

Double Displacement

d)

Combustion

79.

What is the unit for the rate constant (k) for 2nd order reactions?

a)

s-1

b)

M/s

c)

M-1s-1

80.

How does a catalyst speed up a reaction?

a)

Adding more reactant

b)

Lowering the activation energy

c)

Increasing the activation energy

d)

Increasing binding energy

81.

___________ are produced in one step and used up in a later step and __________________ are present and unchanged in the reactants and the products

a)

intermediates, catalysts

b)

catalysts, intermediates

82.

If a “reaction profile” has a taller ‘hill’ (or activation energy) then the reaction is ____________________?

a)

Faster

b)

Slower

83.

What is the half life equation for a first order reaction?

a)

.693/k

b)

t-k

c)

k/.693

d)

rate = k[A]

84.

What are the 2 characteristics that an effective collision must have? SELECT TWO

a)

Enough energy to overcome Ea

b)

Molecules in the correct orientations

c)

High enough temperature

d)

Apporpriate intermediates present

85.

What is the rate law for the reaction with this slow elementary step? A + A --> B + B

a)

rate = k[A]2

b)

rate = k[B]2

c)

rate = k[A][B]

d)

rate = k[A]

86.

What is the rate law for the reaction with this slow elementary step? A --> B + C

a)

rate = k[A]2

b)

rate = k[B]2

c)

rate = k[A][B]

d)

rate = k[A]

87.

What is the rate law for the reaction with this slow elementary step? A + 2B --> D + C

a)

rate = k[A]2

b)

rate = k[A][B]2

c)

rate = k[A][B]

d)

rate = k[A]

88.

What is NOT a way to speed up a reaction

a)

Add a catalyst

b)

Decrease the volume

c)

Increase the concentration of reactants

d)

Increase surface area of the solid

e)

Decrease the pressure

89.

Which curve represents the most particles in this Maxwell-Boltzmann curve (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

They all have the same number of particles

90.

Which curve in this Maxwell-Boltzmann distribution represents the highest proportion of particles moving the fastest (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

All particles are moving at the same speed

91.

Which curve in this Maxwell-Boltzmann distribution would represent the a gas with the highest molar mass?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

92.

What order of reaction has a half-life that does not change regardless of the initial concentration?

a)

Zero

b)

First

c)

Second

d)

Third

93.

Losing electrons is ________________, gaining electrons is ________________

a)

oxidation, reduction

b)

reduction, oxidation

94.

In an exothermic reaction, the sign of ΔH is ____ and the reaction feels ______

a)

(-), hot

b)

(+), hot

c)

(-), cold

d)

(+), cold

95.

In an endothermic reaction, the sign of ΔH is ____ and the reaction feels ______

a)

(-), hot

b)

(+), hot

c)

(-), cold

d)

(+), cold

96.

Freezing is an _________________________ process

a)

Endothermic

b)

Exothermic

97.

Vaporizing is an _________________________ process

a)

Endothermic

b)

Exothermic

98.

What are the coefficients?

a)

1; 2; 1; 2

b)

2; 1; 2; 1

c)

4; 2; 1; 4

d)

1; 4; 2; 2

99.

Breaking bonds is _________________. Forming bonds is ______________________

a)

endothermic, exothermic

b)

exothermic, endothermic

100.

ΔHrxn = ΔH_________________ − ΔH_________________

a)

products, reactants

b)

reactants, products

101.

If a reaction is exothermic, then the bonds formed in the products are ___________________ than the reactant bonds.

a)

stronger/more stable

b)

weaker/less stable

102.

If a reaction is endothermic, then the bonds formed in the products are ___________________ than the reactant bonds.

a)

stronger/more stable

b)

weaker/less stable

103.

According to Hess' Law, if you double the coefficients of a reaction, ΔH will ________________________

a)

Stay the same

b)

Double

c)

Quadruple

d)

Halve

104.

According to Hess' Law, if you reverse a reaction, ΔH will ________________________

a)

Change signs

b)

Double

c)

Be inversed

d)

Halve

105.

_____ Hydrogen-Hydrogen single bond/s are broken and _____ Carbon-Hydrogen single bond/s formed

a)

6; 8

b)

2; 8

c)

2; 10

d)

2; 10

106.

_____ Carbon-Carbon single bond/s are formed

a)

6

b)

2

c)

3

d)

10

107.

Bond enthalpy is the amount of energy is takes to break __________ of a bond.

a)

one mole

b)

one gram

c)

the activation energy

d)

the binding energy

108.

This reaction is ____________________ because energy is _____________

a)

endothemic, absorbed

b)

exothermic, released

c)

endothermic, absorbed

d)

endothermic, released

109.

There are two Carbon(graphite) in the final equation. We should ________ the ΔH of the first sub-reaction.

a)

Double

b)

Halve

c)

Take the inverse of

d)

Reverse the sign of

110.

We need to reverse one of the equations.

a)

True

b)

False

111.

Heat is measure in K or °C

a)

True

b)

False

112.

The particles under the purple curve (middle) have an average Kinetic Energy of 500K

a)

True

b)

False

113.

The particles under the purple curve (middle) all have a temperature of 500K

a)

True

b)

False

114.

What are the units of ΔHrxn?

a)

kJ

b)

J

c)

kJ/mol

d)

J/mol

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