Unit 6: Electrons in Atoms

Question 1

JJ Thomson’s model?

Answer 1

Plum pudding model

Question 2

What does Rutherford Model show?

Answer 2

most of the mass in nucleus and e- in empty space

Question 3

Bohr Model

Answer 3

e- in concentric orbit around nucleus and e- exists in energy levels

Question 4

What are the energy levels like closest to the nucleus?

Answer 4

low energy levels

Question 5

What are the energy levels like farthest from the nucleus?

Answer 5

high energy levels

Question 6

Electron Configuration

Answer 6

Lists the SUBLEVELS (or energy levels) filling with electrons in order of increasing energy

Question 7

What does the first number represent in a sublevel

Answer 7

energy level (the row)

Question 8

What does the letter represent in a sublevel

Answer 8

type of orbital

Question 9

What does the superscript represent in a sublevel

Answer 9

number of electrons

Question 10

Periods on the periodic table are…

Answer 10

rows

Question 11

What are the types of atomic orbitals?

Answer 11

s, p, d, f

Question 12

Energy Levels

Answer 12

regions around the nucleus where electrons are likely to be moving

Question 13

Where is the s orbital on the periodic table?

Answer 13

first 2 columns (and Helium)

Question 14

Where is the p orbital on the periodic table?

Answer 14

last 6 columns

Question 15

Where is the d orbital on the periodic table?

Answer 15

in the middle of

Question 16

What energy level does the d orbital begin with on the periodic table?

Answer 16

3

Question 17

How many electrons in the s orbital?

Answer 17

2

Question 18

How many electrons in the p orbital?

Answer 18

6

Question 19

How many electrons in the d orbital?

Answer 19

10

Question 20

How many electrons in the f orbital?

Answer 20

14

Question 21

What energy level does the f orbital start from?

Answer 21

4

Question 22

Standard Notation of Electron Configuration

Answer 22

ex. 1s2 2s2 2p6

Question 23

Shorthand Configuration

Answer 23

standard Notation that starts with the nearest noble gas before the desired element

ex. [Ar] 4s2

Question 24

Orbital Diagrams: Box Configuration rules

Answer 24

each box contains 2 electrons

electrons are arrows

arrows are paired in opposite directions

each orbital must be labeled

ex.) 3 boxes for p orbital, 5 boxes for d orbital

Question 25

How many electrons can each energy level hold? (Starting from 1)

Answer 25

2, 8, 18, 32

Question 26

What orbitals are in energy level 1?

Answer 26

s

Question 27

What orbitals are in energy level 2?

Answer 27

s, p

Question 28

What orbitals are in energy level 3?

Answer 28

s, p, d

Question 29

What orbitals are in energy level 4?

Answer 29

s, p, d, f

Question 30

Aufbau Principle

Answer 30

fill up the lowest energy levels and orbitals first

Question 31

Pauli's Exclusion Principle

Answer 31

Electrons MUST have opposite spins in orbitals (arrows pointing in opposite directions)

Question 32

Hund's Rule

Answer 32

place one electron in each orbital (with the same spin) and then pair them up

Question 33

Valence Electrons

Answer 33

Electrons on the outermost shell (the highest energy level)

Question 34

Positive ion

Answer 34

Cation

Question 35

Cation

Answer 35

Positive Ion

Question 36

Negative Ion

Answer 36

Anion

Question 37

Anion

Answer 37

Negative Ion

Question 38

______ lose valence electrons

Answer 38

metals

Question 39

How do you identify the valence electrons and cation symbol?

Answer 39

The highest energy level with electrons indicate the valence electrons Number of valence electrons = amount of positiveccharge ex) 3s2 - 2 val = Mg2+

Question 40

______ gain electrons

Answer 40

non-metals

Question 41

Octet

Answer 41

A full outer shell of electrons (8)

Question 42

How to identify anions and their valence electrons

Answer 42

Valence electrons is the highest energy level's (number) electrons how many electrons needed to complete an octet = the negative charge ex) 3s2 3p5 - 7 val - Cl- (because one less than 8)