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Sem 2 Final Review

Total questions: 54

Worksheet time: 1hrs 14mins

Name
Class
Date
1.

The number of wavelengths that pass a point per unit of time is:

a)

frequency

b)

wavelength

c)

longitudinal

d)

transverse wave

2.

What is it called when an electron is gaining energy after it has been exposed to a photon (energy) and becomes excited?

a)

Emission

b)

Absorption

c)

Transmission

d)

Energy

3.

What is it called when an electron loses energy and falls back to the ground state, giving off the photon (light)?

a)

Emission

b)

Absorption

c)

Transmission

d)

Energy

4.

What causes electrons to become excited?

a)

Nothing, it just happens

b)

The electron loses energy by absorbing a photon

c)

The electron gains energy by absorbing a photon

d)

Excited electrons don't exist

5.

What is the wavelength of a wave of light that has a frequency of 2.5 x 1013 Hz?

a)

12 m

b)

.000012 m or 1.2x10-5 m

c)

1.2 m

d)

83,333.33 m or 8.33x104 m

6.

What is the energy of a 3.5 Hz wave?

a)

2.32x10-33 J

b)

2.32 J

c)

5.68x10-26 J

d)

85,714,285.7 J

7.

A photon of light has a wavelength of 2.5 x 10-7 m. Calculate the frequency of this photon.

a)

1.2 x 1015 Hz

b)

1.2 x 1015 m

c)

8.33 x 10-16 Hz

d)

8.33 x 10-16 m

8.

Given a wavelength of 9.7x10-3 m, calculate the ionization energy the of this photon.

a)

2.05 x 10-23 m

b)

3.09 x 1010 m

c)

2.05 x 10-23 J

d)

3.09 x 1010 J

9.

What is the energy of a 5.66 x 108 Hz wave?

a)

3.75x10-24 J

b)

3.75x10-25 J

c)

8.54x1041 J

d)

8.54

10.

What is the energy of a 4.2x10-6 m wave?

a)

7.47x10-20 J

b)

4.74 J

c)

4.74x10-20 J

d)

None of the above

11.

___________ is what is being dissolved in a solution.

a)

Solute

b)

Solvent

c)

Precipitate

d)

Water

12.

What is a colligative property?

a)

Something that depends on the amount of water used

b)

Something that depends on the amount of solute dissolved

c)

Something that does not depend on anything... its just that way

13.

How does water arrange around ions in solution?

a)

The positive hydrogens arrange around the positive ion

b)

The positive hydrogens arrange around the negative ion

c)

The negative oxygens arrange around the positive ion

d)

The negative oxygens arrange around the negative ion

14.

What are 3 methods to increase the rate of dissolution/dissolving?

a)

Particle Size

b)

Temperature

c)

Evaporation

d)

Agitation

e)

Arugula

15.

What is the main unit that differs between molarity and molality?

a)

Molarity uses kg, Molality uses L

b)

Molarity uses L, Molality uses kg

c)

Molarity uses moles, Molality uses Moles

d)

Nothing

16.

What is this image representing?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Insoluble

17.

What is this image representing?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Insoluble

18.

What is this image representing?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Insoluble

19.

What are the particles on the bottom called?

a)

Insaturation

b)

Precipitate

c)

Particles

d)

Solution

20.

_____________ does the dissolving.

a)

solute

b)

solvent

c)

precipitate

d)

salt

21.

In 100g of water, if I have 2.0g of CH4 at 30 degrees... is it saturated, unsaturated, or saturated with a precipitate?

a)

saturated

b)

unsaturated

c)

saturated with a precipitate

22.

Based on the trends of each chemical as temp increases, what can we assume about its state of matter?

a)

They are likely solids

b)

They are likely gases

c)

They are likely liquids

d)

There is no way to know

23.

In 100g of water, what is the solubility of K2Cr2O7 (purple line) at 90 degrees?

a)

70 g

b)

140 g

c)

50 g

d)

65 g

24.

In 100g of water at 40 degrees, I put 45 grams of KNO3 into the solution.... is this solution saturated, unsaturated, or saturated with a precipitate?

a)

saturated

b)

unsaturated

c)

saturated with precipitate

25.

What is the solubility of NaNO3 at 10 degrees in 200g of water?

a)

40 g

b)

80 g

c)

160 g

26.

What is this equation?

a)

molality

b)

solubility

c)

molarity

d)

stoichiometry

27.

What is this equation?

a)

molality

b)

solubility

c)

molarity

d)

stoichiometry

28.

Because of the partial positive and partial negative charges, water is considered to be

a)

nonpolar

b)

wet

c)

polar

d)

ionic

29.

What numbers on the pH scale represent acidic solutions?

a)

0-7

b)

7

c)

7-14

30.

What side of the pH scale contains the highest concentration of hydroxide ions?

a)

Left

b)

Middle

c)

Right

31.

What number on the pH scale has equal concentrations of H+ and OH- ?

a)

1

b)

7

c)

14

d)

None

32.

As pH decreases, the H+ concentration...

a)

increases

b)

decreases

c)

stays the same

33.

What are the products of an acid/base reaction?

a)

Salt

b)

Water

c)

Salt & Water

d)

Acid & Base

34.

According to the definition of a base, bases produce....

a)

hydrogen

b)

hydroxide

c)

water

d)

carbonic acid

35.

What is the equation you use to determine an unknown concentration during a titration?

a)

maVb = mbVa

b)

MaVa = MbVb

c)

MaVb = MbVa

d)

maVa = mbVb

36.

If I have a pH of 9.5, what is the concentration of hydrogen ions?

a)

10 x 10-9.5

b)

1 x 109.5

c)

1 x 10-9.5

d)

9.5 x 10-9.5

37.

The concentration of hydrogen ions is 1x10-3 , what is the pOH?

a)

11

b)

3

c)

14

d)

1

38.

Is KOH an acid or a base?

a)

acid

b)

base

c)

neither

39.
This type of  reaction occurs when a heavy nucleus, such as U-235, splits into two or more parts.
a)
Fission
b)
Fusion
c)
Chain reaction
d)
synthesis
40.

Nuclear _______________ is when a large unstable nucleus breaks into two smaller nuclei.

a)

Fusion

b)

Fission

41.
Arrange in order of increasing ability to penetrate matter.
a)
Beta, gamma, alpha
b)
Alpha, gamma, beta
c)
Gamma, beta, alpha
d)
Alpha, beta, gamma
42.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
43.
Complete the nuclear equation and determine the type of decay that is occurring in this reaction. 
a)
alpha
b)
beta
c)
gamma
d)
none
44.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
45.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
46.
Calculate the molar mass of Mg(OH)2.
a)
33.2 g/mol
b)
41.3 g/mol
c)
86.9 g/mol
d)
58.3 g/mol
47.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
48.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
49.
What is the electron configuration for nitrogen?
a)
1s2 2s2 2p3
b)
1s2 2s3 2p2
c)
1s2 2s3 2p1
d)
1s2 2s2 2p2 3s1
50.
Which of the following rules requires that each of the p orbitals at a particular energy level receive one electron before any of them can have two electrons?
a)
the Pauli exclusion principle
b)
Hund's rule.
c)
the Aufbau principle.
d)
the quantum rule.
51.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
52.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
53.
The exponent or superscript in an electron configuration tells us
a)
the number of positions of that orbital.
b)
the distance from the nucleus or level.
c)
the number of electrons in that orbital.
d)
the number of electrons in the atom.
54.
How many valance electrons are in 1s22s22p63s2
a)
4 ve
b)
2 ve
c)
8 ve
d)
6 ve

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