Free Printable Unit 4 Review S2025

Worksheets

Unit 4 Review S2025

Total questions: 32

Worksheet time: 22mins

Name

Class

Date

Which of the following is a statement of the law of conservation of energy?

Energy can be created and destroyed.

Energy cannot be created or destroyed, only transformed.

Energy is always lost as heat.

Energy is only conserved in closed systems.

What is the trend in atomic radius as you move from left to right across a period in the periodic table?

It increases.

It decreases.

It remains constant.

It fluctuates randomly.

Calculate the amount of heat absorbed by 50 g of water when its temperature increases from 20°C to 30°C. (Specific heat capacity of water = 4.18 J/g°C)

209 J

418 J

2090 J

4180 J

Which of the following is the correct electron configuration for a neutral atom of oxygen?

$1s^2 2s^2 2p^4$

$1s^2 2s^2 2p^6$

$1s^2 2s^2 2p^3$

$1s^2 2s^2 3p^4$

Which type of bond involves the transfer of electrons from one atom to another?

Covalent bond

Ionic bond

Metallic bond

Hydrogen bond

Explain why the ionization energy generally increases across a period in the periodic table.

Electrons are added to the same energy level, increasing nuclear charge.

Electrons are added to higher energy levels, decreasing nuclear charge.

Electrons are removed from the same energy level, decreasing nuclear charge.

Electrons are added to lower energy levels, increasing nuclear charge.

A 100 g sample of a metal absorbs 500 J of heat, and its temperature rises by 10°C. What is the specific heat capacity of the metal?

0.5 J/g°C

1.0 J/g°C

5.0 J/g°C

10.0 J/g°C

Which of the following elements has the highest electronegativity?

Fluorine

Oxygen

Nitrogen

Chlorine

Describe the difference in electron sharing between ionic and covalent bonds.

Ionic bonds involve equal sharing; covalent bonds involve transfer.

Ionic bonds involve transfer; covalent bonds involve equal sharing.

Ionic bonds involve unequal sharing; covalent bonds involve transfer.

Ionic bonds involve equal sharing; covalent bonds involve unequal sharing.

10.

Predict the molecular shape of $\text{PH}_3$ using VSEPR theory.

Pyramidal

Trigonal planar

Tetrahedral

Bent

11.

Which of the following statements best describes the wave mechanical model of the atom?

Electrons orbit the nucleus in fixed paths.

Electrons are found in specific energy levels.

Electrons exist in probability clouds called orbitals.

Electrons are stationary around the nucleus.

12.

Which of the following is a characteristic of covalent compounds?

High melting and boiling points

Conduct electricity in solution

Formed between metals and nonmetals

Low melting and boiling points

13.

Explain why metals tend to lose electrons and nonmetals tend to gain electrons in chemical reactions.

Metals have high ionization energies; nonmetals have low ionization energies.

Metals have low ionization energies; nonmetals have high ionization energies.

Metals have high electronegativities; nonmetals have low electronegativities.

Metals have low electronegativities; nonmetals have high electronegativities.

14.

What is the primary reason for the increase in atomic size as you move down a group in the periodic table?

Increase in nuclear charge

Increase in electron shielding

Decrease in nuclear charge

Decrease in electron shielding

15.

Which of the following is the correct Lewis structure for water ( $\text{H}_2\text{O}$ )?

$\text{H}-\text{O}-\text{H}$ with two lone pairs on O

$\text{H}=\text{O}=\text{H}$

$\text{H}-\text{O}-\text{H}$ with no lone pairs on O

$\text{H}=\text{O}-\text{H}$

16.

A chemical reaction releases 150 kJ of energy. According to the conservation of energy, what happens to this energy?

It is destroyed.

It is absorbed by the surroundings.

It is converted into mass.

It remains in the system.

17.

Which of the following best explains why ionic compounds are typically solid at room temperature?

They have strong covalent bonds.

They have strong electrostatic forces between ions.

They have weak intermolecular forces.

They have low melting points.

18.

Which of the following elements is most likely to form a cation?

Sodium

Chlorine

Oxygen

Nitrogen

19.

Which of the following best describes the electron configuration of a noble gas?

Completely filled s and p orbitals

Completely filled s orbitals only

Partially filled p orbitals

Partially filled s and p orbitals

20.

Which of the following molecules is polar?

$\text{CO}_2$

$\text{CH}_4$

$\text{H}_2\text{O}$

$\text{N}_2$

21.

Explain why $\text{CO}_2$ is a nonpolar molecule despite having polar bonds.

The molecule is linear, and the dipoles cancel each other out.

The molecule is bent, and the dipoles reinforce each other.

The molecule is tetrahedral, and the dipoles cancel each other out.

The molecule is trigonal planar, and the dipoles reinforce each other.

22.

If a little packet of energy comes their way, (a) may use it to jump to the next higher orbit or (b) (that is, farther away from the nucleus). Or, they may fall back to a lower orbit (closer to the nucleus), and give up a little packet of energy or (c) . Depending on the wavelength, you may see this as a particular (d)

Choose from the below words

electrons

energy level

photon

color

protons

neutrons

mass

frequency

23.

A 45-g aluminum spoon (specific heat 0.88 J/g °C) at 24 °C is placed in 180 mL (180 g) of coffee at 85 °C and the temperature of the two become equal.

What is the final temperature when the two become equal? Assume that coffee has the same specific heat as water (4.18).

Use two decimal places.

24.

This picture shows a...

Ionic Bond

Covalent Bond

Both bonds

Neither bond

25.

What is the primary factor that determines the polarity of a molecule?

The shape of the molecule and the electronegativity of its atoms

The number of atoms in the molecule

The atomic mass of the central atom

The total number of electrons in the molecule

26.

Which of the following elements is most likely to form an anion?

Fluorine

Aluminum

Calcium

Potassium

27.

Which of the following molecules has a bent molecular shape?

$\text{BF}_3$

$\text{CH}_4$

$\text{CO}_2$

$\text{H}_2\text{O}$

28.

Which of the following best describes the electron configuration of an alkali metal?

Partially filled p orbital

Completely filled d orbitals

Partially filled s orbital

Completely filled s and p orbitals

29.

Frequency and Energy of a wavelength are (a) related

30.

Which of the following best describes the trend in electronegativity as you move down a group in the periodic table?

It fluctuates randomly

It remains constant

It decreases

It increases

31.

When all electrons are in the lowest possible energy levels, an atom is said to be in its (a) . When an atom absorbs energy so that its electrons are “boosted” to higher energy levels, the atom is said to be in an (b) .

Choose from the below words

GROUND STATE

EXCITED STATE

ionized state

covalent state

32.

Classify each process as exothermic or endothermic. Explain. The system is underlined in each example.

a)Your hand gets cold when you touch ice. (a)

b)The ice gets warmer when you touch it. (b)

c)Water boils in a kettle being heated on a stove. (c)

d)Water vapor condenses on a cold pipe. (d)

e)Ice cream melts. (e)

Choose from the below words

exothermic

endothermic

no change in energy

Reset

Unit 4 Review S2025

Total questions: 32

Worksheet time: 22mins

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