unit 2 test

Question 1

s sub-level:

Answer 1

Shaped like a sphere. Holds 2 electrons.

Question 2

p sub-level:

Answer 2

Shaped like a dumbbell (two lobes). Holds 6 electrons.

Question 3

d sub-level:

Answer 3

Shaped like a cloverleaf. Holds 10 electrons.

Question 4

Size Changes:

Answer 4

As energy levels increase (1, 2, 3, etc.), the size of these shapes gets bigger because the electrons are farther from the nucleus.

Question 5

Rules for Filling Electrons

Answer 5

• Fill Lowest Energy First
• Only 2 Electrons per Orbital
• Spread Out Before Pairing

Question 6

Principle Energy Level:

Answer 6

The main energy level of an atom (1, 2, 3, etc.).

Question 7

Sub-level

Answer 7

The types within each level (s, p, d, f)

Question 8

Orbitals:

Answer 8

Spaces within each sub-level where electrons are likely to be found. Each orbital can hold 2 electrons.

Question 9

Light Release from atoms is when …

Answer 9

When electrons absorb energy, they jump to higher energy levels. When they fall back down, they release light.

Question 10

when Wavelength and Color is released from atoms this is what happens

Answer 10

Different amounts of energy create different colors because they have different wavelengths and frequencies.

Question 11

Types of Light

Answer 11

• Radio Waves: Longest wavelength, used for radio and TV.
• Visible Light: What we see; colors range from red to violet.
• Ultraviolet (UV): Higher energy than visible light; can cause sunburn.
• X-rays: Used for medical imaging.
• Gamma Rays: Highest energy, used in cancer treatment.

Question 12

What is electron configuration

Answer 12

Shows how electrons are arranged in an atom.

Question 13

What are Valence Electrons:
Give an example

Answer 13

Electrons in the outermost energy level. They determine how an element reacts.
Example: Oxygen’s electron configuration is 1s² 2s² 2p⁴; it has 6 valence electrons

Question 14

Periodic Table Trends –
What is atomic radius
What’s the trend
Why does it do it

Answer 14

Atomic radius is the size of an atom
Trend: Gets smaller across a row (left to right) and larger down a group (top to bottom).
Why?: More protons pull electrons closer across a row; more energy levels make atoms bigger down a group.

Question 15

Periodic Table Trends –
What is Ionization Energy:
What is its trend?
Why does it do it

Answer 15

Energy needed to remove an electron.
Trend: Increases across a row, decreases down a group.
Why?: Harder to remove electrons when atoms are smaller (across) and easier when atoms are larger (down).

Question 16

Periodic Table Trends –
What is Electronegativity:
What is its trend?
Why does it do it

Answer 16

Ability of an atom to attract electrons.
Trend: Increases across a row, decreases down a group.
Why?: Smaller atoms have a stronger pull on electrons than larger ones.

Question 17

Orbital Diagrams:

Answer 17

Draw each orbital as a line, and add arrows (↑↓) for each electron.

Question 18

Electron Configurations:

Answer 18

Use numbers and letters to show the order of electrons (e.g., 1s² 2s² 2p⁶).

Question 19

1s² 2s² 2p⁶).
Shorthand (Noble Gas Notation):

Answer 19

1s² 2s² 2p⁶).
Shorthand (Noble Gas Notation):

Question 20

d4 and d9 Exceptions:

Answer 20

Some d sub-levels are more stable when half-full or nearly full, so they “borrow” an electron from the previous s orbital.