Quiz Unit 2

Question 1

3 Types of Subatomic Particles

Answer 1

Proton
Electron
Neutron

Question 2

Neutral Atoms vs Ions

Answer 2

Atoms - # of protons = # of electons
+ no net charge

Ions - charged atoms
Pos or neg
caused by loss/gain of electrons

Question 3

Isotopes of the same element have different _____ because ________

Answer 3

mass #s
they have different #s of neutrons

Question 4

Mass Number equation

Answer 4

P (protons) + n (neutrons)

Question 5

What is what in Nuclear symbol notation
#
X
#

Answer 5

Mass #
Element symbol
Atomic #

Question 6

What is what in Isotopes
ex: chlorine-35

Answer 6

35 = mass #

Question 7

Can atoms of the same element have different #s of protons

Answer 7

no, protons are the identity

Question 8

Can atoms of the same element have different # of electrons

Answer 8

yes, changes the charge (ions)

Question 9

Can atoms of the same element have different # of nuetrons

Answer 9

yes, isotopes

Question 10

Stable isotopes

Answer 10

stable ratio of protons to neutrons

Question 11

Radioisotopes

Answer 11

have unstable nuclei and become more stable through nuclear reactions

Question 12

Synthetic elements

Answer 12

man made
have no isotopes
whole # for their atomic mass

Question 13

Why is atomic mass a weighted average?

Answer 13

because average atomic mass depends on the average of each isotope and the % of natural abundance

Question 14

Calculating Atomic Mass equation

Answer 14

AAM = (mass x % abundance) + (mass x % abundance)
___________________________
100

Question 15

Unit for AAM

Answer 15

grams (g) or atomic mass unit (amu)

Question 16

Protons identify the _____
Electrons identify the ______

Answer 16

Identity
Behavior

Question 17

Electrons exist in…

Answer 17

Principal energy levels

Question 18

there are __ principle energy levels

Answer 18

7

Question 19

n=1

Answer 19

closet to the nucleus
lowest energy level

Question 20

n=7

Answer 20

farthest from nucleus
highest energy level

Question 21

An electron must ______ specific amounts of energy to move from one energy level to another

Answer 21

absorb/emit

Question 22

It requires ___________ for an electron to move between energy levels farthest from each other

Answer 22

more energy

Question 23

a quantum of energy is the _________ required to move an electron from one energy level to another

Answer 23

amount of energy

Question 24

n=1 is the _______ from other energy levels

Answer 24

most separated

Question 25

Within each energy level there are different _____

Answer 25

sublevels

Question 26

There are ___ types of sublevels ___,____,____,____

Answer 26

4 s, p, d, and f

Question 27

each energy sublevel corresponds to 1 or more differently shaped ______

Answer 27

atomic orbitals

Question 28

An atomic orbital describes the ________ of finding an electron in the region around the nucleus

Answer 28

probability

Question 29

An orbital can hold _____ electrons

Answer 29

2

Question 30

# of atomic orbitals s orbital # of atomic orbitals shape max electrons

Answer 30

1 atomic orbital sphere 2 max electrons

Question 31

# of atomic orbitals p orbital # of atomic orbitals shape max electrons

Answer 31

3 atomic orbitals dumbbell 6 max electrons

Question 32

f orbital # of atomic orbitals max electrons

Answer 32

7 max orbitals 14 max electrons

Question 33

d orbital # of atomic orbitals shape max electrons

Answer 33

5 atomic orbitals 4 leaf clover 10 max electrons

Question 34

Electron Configuration

Answer 34

arrangement of electrons in a atom

Question 35

Aufbau Principle (filling in)

Answer 35

electrons fill sublevels in order of lowest to highest

Question 36

What is what in Electron Configuration # (s, p, d, f)#

Answer 36

Principal energy level (n=1) (sublevel type) # of electrons in that sublevel

Question 37

Core Notation/short-hand configuration

Answer 37

[noble gas in row before] #(sublevel type)# etc

Question 38

Pauli Exclusion Principle (spins)

Answer 38

when electrons exist in a pair they have opposite spins

Question 39

Hunds rule (empty bus seat rule)

Answer 39

for p/d/f sublevels the electrons fill the empty orbitals before pairing

Question 40

1s2 2s2 2p4 What is the total # of electrons what do arrows look like

Answer 40

8 total electrons ^,, ^,, ^,, ^ ^

Question 41

What is the maximum number of electrons in the second principal energy level?

Answer 41

6

Question 42

How many energy sublevels are in the second principal energy level?

Answer 42

2

Question 43

When an electron moves from a lower to a higher energy level, the electron ____

Answer 43

absorbs a quantum of energy

Question 44

The quantum mechanical model describes the allowed ____ an electron can have

Answer 44

orbitals / energies

Question 45

Each atomic orbital has a different _____ and ______

Answer 45

shape and energy

Question 46

Within a principal energy level, there are energy _____

Answer 46

sublevels