Final Review #1

Unit 2 Review

Coulomb's Law

Multiple Choice

Which of the following best describes the impact of distance on the attractive force between particles?

• As the distance between oppositely charged particles increases, the force of attraction between the particles increases

• As the distance between oppositely charged particles increases, the force of attraction between the particles decreases

• There is no relationship between the distance between two oppositely charged particles and their force of attraction.

• As the distance between oppositely charged particles decreases, the force of attraction between the particles decreases

Multiple Choice

As you move from the top of Group #1 from Li to K how does the distance between the outermost electron and the nucleus change?

• the outermost electron is further away in the larger atom (potassium)

• the outermost electron is closer to the larger atom (potassium)

• the outermost electron is further away in the smaller atom (lithium)

• the outermost electron is closer away in the smaller atom (lithium)

Multiple Choice

Finish this sentence: As more protons are added ,the attractive force on the electron _____________.

• increases

• decreases

• stays the same

• tu eres loco, Hagerman

Multiple Select

USE THE PERIODIC TABLE above to determine which element whose atoms will have a stronger attractive force between their outermost electron(s) and the nucleus.

• Ba

• Ca

Multiple Select

USE THE PERIODIC TABLE above to determine which element whose atoms will have a stronger attractive force between their outermost electron(s) and the nucleus.

• Ar

• Ge

• Kr

Multiple Select

USE THE PERIODIC TABLE above to determine which element whose atoms will have a stronger attractive force between their outermost electron(s) and the nucleus.

• Bi

• As

• N

• Sb

Multiple Select

USE THE PERIODIC TABLE above to determine which element whose atoms will have a stronger attractive force between their outermost electron(s) and the nucleus.

• Ga

• P

• He

• O

Open Ended

When comparing elements in the same row (PERIOD) of the periodic table, which factor—distance to the nucleus or number of protons in the nucleus—seems to be the dominant factor for determining the attractive force between the outermost electron(s) and the nucleus? Explain.

Electron Energy, Light, EMS

Multiple Choice

Do all colors of light travel at the same speed?

• yes

• no

Multiple Choice

Do all colors of light have the same energy?

• yes

• no

Multiple Choice

Even though all colors of light travel at the same speed, they all have different amounts of energy. Which color has the lowest energy of light?

• reds

• violets

• greens

• oranges

Multiple Choice

Even though all colors of light travel at the same speed, they all have different amounts of energy. Which color has the highest energy of light?

• Reds

• Oranges

• Blues

• Violets

Multiple Choice

Does this example show a electron light release a high wave or low energy wave?

Would this be more like a violet emission or red emission?

• high / red

• low / red

• high / violet

• low / violet

Multiple Choice

Does this example show a electron light release a high wave or low energy wave?

Would this be more like a violet emission or red emission?

• high / red

• low / red

• high / violet

• low / violet

Multiple Choice

Longer wavelength means _____ frequency

• less

• more

Multiple Choice

Shorter wavelength means _____ frequency

• less

• more

Multiple Choice

More frequency means ______ energy

• more

• less

PES, Electron Configs, Orbital Diagrams

huh?

Multiple Choice

What is the relationship between the ionization energy of an electron and the net attractive force that holds an electron in an atom?

• Ionization energy = attractive force

• Ionization energy > attractive force

• Ionization energy < attractive force

Multiple Choice

How many energy levels are in this PES example of Sulfur?

• 1

• 2

• 3

• 4

Multiple Choice

Why does Sulfur have a higher IE with its first Energy Level compared to Phosphorus?

• The higher amount of protons in Sulfur create a stronger attractive force between the nucleus and first energy level

• The lower amount of protons in Phosphorus create a stronger attractive force between the nucleus and first energy level

• The last energy level takes all the energy from the Phosphorus's first energy level

Multiple Choice

write this electron configuration:

Chromium (Cr)

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁴

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵

• 1s⁴ 2s² 2p⁴ 3s² 3p⁶ 4s² 3d⁴

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s⁶

Multiple Select

Check ALL that apply for the correct electron configuration:

Bromine (Br)

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁵ 3d¹⁰

• [Ar] 4s² 3d¹⁰ 4p⁵

• [Zn] 4p⁵

Make sure you can connect all four types of models!

Periodic Trends, Ions, Valence Electrons

Multiple Choice

Using what you know about Coulombic attraction and atomic structure, choose the statement that best describes the reason for the trend in atomic radius down a group.

• As you move down a group, more protons are added to the nucleus of an atom, increasing Coulombic attraction.

• As you move down a group, the Coulombic attraction between the nucleus and valence electrons decreases.

• As you move down a group, the valence electrons are added to higher energy level and are farther from the nucleus.

• As you move down a group, the core electrons are more attracted to the nucleus.

Multiple Choice

In general, what is the trend in atomic radius as you go across a period? Hint: Rows on the periodic table are called periods.

• Atomic radius increases.

• Atomic radius decreases.

• Atomic radius stays constant.

Multiple Choice

What does ionization energy measure?

• The distance from the nucleus to the valence electrons.

• The distance from the nucleus to electrons in the first energy level.

• The amount of energy needed to remove a valence electron from an atom.

• The amount of energy needed to move an electron from the first energy level to a higher energy level.

Multiple Choice

In general, what is the trend in ionization energy as you go down a group? Hint: Compare the ionization energies of helium, neon, argon, krypton, xenon, and radon.

• Ionization energy increases.

• Ionization energy decreases.

• Ionization energy stays constant.

Open Ended

How might you be able to determine then number of valence electrons in an atom by looking at the electron configuration for an element?

Multiple Choice

How many valence electrons are in this configuration?

1s² 2s² 2p⁶ 3s²

• 2

• 8

• 4

• 1

Multiple Choice

How many valence electrons are in this configuration?

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p³

• 5

• 13

• 2

• 3

Open Ended

compare and contrast mass number and atomic mass.

Multiple Choice

Which of the following best describes the isotopes of Boron?

• There are more isotopes of Boron-11 in nature than there are isotopes of Boron-10

• There are more isotopes of Boron-10 in nature than there are isotopes of Boron-11

• The number of isotopes of Boron-10 in nature is the same as Boron-11

• It is impossible to tell which isotope is more abundant in nature