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Test 4 Review 2025 S1

Total questions: 37

Worksheet time: 6hrs 10mins

Name
Class
Date
1.

1 mole of gas occupies what volume at STP?

a)

22.4 L

b)

6.02 x 1023 L

2.

Convert: -30 C to K

a)

243 K

b)

-303 K

c)

303 K

d)

-243 K

3.

If a gas is at 0.95 atm, how many kPa is this?

a)

0.35 kPa

b)

1.07 kPa

c)

96 kPa

d)

400,025 kPa

4.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
5.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
6.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
7.
Boyle's law : When _______ is held constant, the pressure and volume of a gas are ________  proportional
a)
temperature,  equally
b)
mass, inversely
c)
temperature, inversely
d)
mass, equally
8.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
9.

According to the Plum Pudding Model, what is the structure of an atom?

a)

Negatively charged sphere with positively charged electrons embedded in it.

b)

Positively charged sphere with negatively charged electrons embedded in it

c)

Positively charged sphere with positively charged electrons embedded in it.

d)

Negatively charged sphere with negatively charged protons embedded in it.

10.

Who discovered the electron?

a)

J.J. Thomson

b)

Marie Curie

c)

Isaac Newton

d)

Albert Einstein

11.

What experiment did J.J. Thomson conduct to discover the electron?

a)

Cathode ray tube experiment

b)

Oil drop experiment

c)

Millikan experiment

d)

Rutherford gold foil experiment

12.

Why did Ernest Rutherford and his colleagues perform the Gold-Foil Experiment?

a)

They wanted to test and confirm the Plum-Pudding model

b)

They wanted to test John Dalton's Model

c)

They were looking for electrons

d)

They wanted to come up with their own Atomic Model

13.

What results did Rutherford expect to see if the Plum-Pudding model is correct?

a)

He expected that most of alpha particles would go through a gold-foil and small number of particles would deflect sightly

b)

He expected that most of alpha particles would not go through a gold-foil and will stop on one side of a foil.

c)

He expected that most of alpha particles would ricochet back after hitting a gold-foil

14.

Choose one of the conclusions that Ernest Rutherford made based on the experimental results of his Gold-Foil experiment

a)

He concluded that the atom is indivisible

b)

He concluded that the atom is mostly empty space

c)

He concluded that the atom has neutrons

d)

He concluded that the atom is tightly packed with subatomic particles all mixed together

15.
Tom Brady enjoys balloon animals from the carnival. He just received a balloon giraffe that has an initial temperature of 39.0°C and a volume of 1.28 L. If Gronkowski plays a trick on Tom, and puts his balloon giraffe into the freezer, what would be the new volume of the balloon if the temperature drops down to 8.0°C?
(Don’t forget about what must be done to temperatures!)
a)
1.42 L
b)
6.85 x 104 L
c)
3.78 L
d)
1.15 L
16.

Bill Belichick uses a lot of hairspray to keep his hair looking good while coaching an entire game. If his can of hairspray has an initial temperature of 22°C and a pressure of 128.1 kPa, what would be the final temperature of the gas is the pressure decreases to 116.8 kPa after use?

a)
176 K
b)
322 K
c)
323 K
d)
269 K
17.

A sample of sulfur dioxide occupies a volume of 652 mL at 313 K and 150 kPa. What volume will the sulfur dioxide occupy at STP?


STP = 273 K, 101.3 kPa

a)

1682.6 mL

b)

20.7 mL

c)

492.3 mL

d)

842.1 mL

18.

Atoms only emit light of certain frequencies because...

a)

electrons move continuously

b)

electrons move up energy levels

c)

electrons can only have certain energies

d)

all of these are true

19.

Light of a specific frequency is emitted when...

a)

an electron absorbs energy

b)

an electron moves down an energy level

c)

when an electron gets excited

d)

all of these are true

20.

Consider the following data:

Cu - blue, green, teal

Na - yellow-orange

K - yellow, orange, pink/lavender

Li - red, light red

Sr - deep red

If the unknown color was yellow-orange, which element is most likely the unknown?

a)

Cu

b)

Na

c)

K

d)

Li

21.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
22.

The color of emitted light with the HIGHEST frequency is

a)

violet

b)

green

c)

red

d)

indigo

23.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
24.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
25.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
26.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
27.

Suppose you have two gases numbered 1 and 2.

Which equation represents make the most sense to calculate the total pressure exerted by both gases?

a)

Multiply their pressures :

Ptotal = P1 × P2

b)

Divide their pressures :

Ptotal = P1 ÷ P2

c)

Add their pressures :

Ptotal = P1 + P2

d)

Subtract their pressures :

Ptotal = P1 – P2

e)

Average their pressure :

Ptotal = (P1 + P2)/2

28.
A student collected 100.mL of butane gas from a lighter via water displacement. The gas was collected at 25°C and the external barometric pressure was 1.00atm.  The partial pressure of H2O at 25°C is 23.78mmHg.  What was the number of moles of butane gas collected?
a)
0.00409mol
b)
0.00792mol
c)
0.00396mol
d)
0.00817mol
29.

Find the number of moles of ammonia gas, NH3, produced from a reaction of 4 moles of nitrogen gas at STP with excess hydrogen gas. Assume the pressure and temperature remain constant. (Hint: You will need a balanced chemical equation. Remember your diatomic elements!)

a)
2 mol
b)
8 mol
c)
4 mol
d)
1 mol
30.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
31.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
32.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
33.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
34.
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
35.

The boiling point of a chemical (Ethanol) is 78.40 Degrees Celsius. A Student conducts an experiment and finds the boiling point of 75.0 Degrees Celsius. What is the percent error of the student's measurement?

a)

3.57%

b)

4.3%

c)

96.56%

d)

2.7%

36.

What is the density of an ammonia gas sample (NH3) if the pressure is 0.928 atm and the temperature is 63.0°C?

a)

1.96 g/l

b)

1.18 g/l

c)

1.43 g/l

d)

0.573 g/l

37.

A gas has a mass of 0.62 g occupying 0.24 liters. The pressure is 98.2 kPa and the temperature is 15°C. What is the molar mass of the gas?

a)

56.8 g/mol

b)

37.0 g/mol

c)

63 g/mol

d)

63.0 g/mol

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