Unit 2 - Atomic Concepts - Electrons - Regents

Question 1

Definition of Ions (3)

Answer 1

1. Num. of Protons ≠ Num. of Electrons
2. Number of Electrons Vary
3. Both + and - Charges are Present

Question 2

What makes an Ion an Anion?

Answer 2

More Electrons

Question 3

What makes an Ion a Cation?

Answer 3

Less Electrons

Question 4

What is it called when an electron is in its highest and lowest energy state?

Answer 4

Lowest: Ground State
Highest: Excited State

Question 5

Definition of Emission Spectra (6)

Answer 5

1. e- falls from excited to ground state
2. The E that was gained is released
3. Released E emitted thru electromagnetic radiation as visible light
4. Emitted E shows up as a series of bright bands on a dark background
5. Amount of E Emitted = Amount of E that was Absorbed
6. Bright bands correspond to specific wavelengths of light

The amount of energy absorbed or released during these transitions is quantized, meaning it corresponds to specific values that depend on the energy levels involved. Since energy and wavelength are directly related, the emitted light has a wavelength unique to that transition—this is why each element has a distinct emission spectrum

Question 6

Definition of Absorption Spectra (5)

Answer 6

1. e- jump from ground to excited state
2. Absorbs E from incoming light/radiation
3. Appears as a series of dark bands on a bright background
4. Amount of E Absorbed = Amount of E that will be Emitted
5. Dark bands correspond to the specific wavelengths of the light that was absorbed

Question 7

Why is the elemental spectra is called an element’s fingerprints? How? (6)

Answer 7

1. Spectra is unique to each element
2. Number of protons vary in elements
3. Nuclear pull/attraction between electrons and protons vary
4. Amount of energy for electrons vary
5. Wavelengths from emitted energy vary
6. So, spectra will vary from element to element

Question 8

What is the relationship between energy levels and spectral lines?

Answer 8

1. More Energy Levels
2. More Ways an Electron can Jump
3. More Spectral Lines

Question 9

Relationship between wavelength & frequency to amount of energy

Answer 9

Longer Wavelengths & Lower Frequency =
Less Energy

Shorter Wavelengths & Higher Frequency =
More Energy

Question 10

List colors of visible light in order of increasing energy

Answer 10

Red
Orange
Yellow
Green
Blue
Violet

Question 11

Definition of Photon

Answer 11

Particle of Light

Question 12

What are Valence Electrons? (3)

Answer 12

1. Electrons on Outermost Shell
2. Determine how an element will bond
3. Number of VE affects Chem. Properties of an element

Equal to Group # on Periodic Table

Question 13

What is the Octet Rule? (3)

Answer 13

1. An atom is most stable with 8 VE
2. Atoms will react or bond to fill up shells
3. EVERYONE WANTS STABILITY

Question 14

What is the relationship between noble gases and the octet rule? (5)

Answer 14

1. ALL Noble Gases
2. In Group 18
3. Have 8 VE
4. They are VERY stable/unreactive
5. Exception: He is still stable, but has 2 VE

Question 15

What are Lewis Dot Diagrams? (3)

Answer 15

1. A way of Drawing VE
2. Element Symbol
3. Surrounded by a Maximum of 8 VE

Question 16

Why does a greater transition from energy levels have the most energy?

Answer 16

1. The farther an atom is from the nucleus, the more energy it has
2. Due to the attraction, the closer an electron is to a nucleus, the energy decreases
3. So, the larger jump, the greater difference of energy.

Question 16

How do you draw a lewis dot diagram when the element is an ion? (5)

Answer 16

1. +1, lose an electron
2. -1, add an electron
3. Add Brackets to the element
4. Add the charge to the element
5. If there is more than 8 VE, there will be 0 VE