Unit 2

Question 1

7^3Li^1+
Where is mass number
Where is proton number
Where is charge

Answer 1

top left
bottom left
top right

Question 2

_______ when natural atom loses electrons
________ when a neutral atom gains electrons
________ same protons but different neutrons

Answer 2

cation, anion, isotope

Question 3

What is the difference between mass number and atomic mass?

Answer 3

mass number - sum of protons and neutrons
atomic mass - average weighted mass of the different forms of the same type of atom. on the periodic table

Question 4

Weighted average:
(1st number)(percentage) + (2nd #)(%)/100

Answer 4

This is how the atomic mass is found

Question 5

Carbon - 13, 13 represents the _____________
means
6 protons
6 elections
7 neutrons

Answer 5

mass number

Question 6

________ is what distinguishes an element from another

Answer 6

protons

Question 7

_________ - # of valence electrons
_______ - # of energy levels

Answer 7

columns/groups
rows/periods

Question 8

How many valence electrons:
13, 14, 15, 16, 17, 18

Answer 8

3, 4, 5, 6, 7, 8

Question 9

_______ atoms preference for having 8 electrons in the valence shell

______ and ______ only want 2 electrons

1st shell - ______
2nd shell - ______
3rd shell - ______-

Answer 9

octet rule
hydrogen, helium
2, 8, 18

Question 10

Lewis structure/dot structure only shows the __________

Answer 10

valence electrons

Question 11

an electron must _________ to move to a HIGHER energy level
________ are the origin of atomic emission spectrum
_________ specific pattern of colored lines that is seen when the light emitted from a smile of identical superheated atoms is viewed through a prism

Answer 11

gain energy
energy levels
atomic emission spectrum

Question 12

When an electron moves up a level is _________
When it falls down levels it ____________
The more energy levels the electron travels, the more energy

Answer 12

absorbs energy
releases energy

Question 13

Red ————> Purple
_______ —————–> ________

Answer 13

least energy, long wavelength
most energy, short wavelength

Question 14

_______ the distance between the adjacent peaks of a wave
_______ # of wavelengths that pass a designated point in one second

Answer 14

wavelength
frequency

Question 15

wavelength and frequency have a _______ relationship
E =
c =
_________ light behaves as a particle and a wave

Answer 15

inverse
energy
speed of light
wave particle duality

Question 16

_____ cases the energy to jump energy levels
it falls back to ________
an electron needs more energy to get farther away from where it started

Answer 16

excitation
base level

Question 17

electrons remain in their energy levels unless something causes them to move to a different level
the amount of energy released is equal to the ______________

Answer 17

difference in energy between the two levels

Question 18

light is a form of _________

Answer 18

electromagnetic radiation

Question 19

quantum mechanical model determines:
____________
__________

Answer 19

allowed energies an electron can have
how likely to find the electron in various locations

Question 20

________ region where electrons are present
n = _______

Answer 20

atomic orbital
energy level

Question 21

energy sub levels: ____, ___, ____, ____

1s^2 what do each part represent?

Answer 21

s, p, d, f,
1 = energy level
s = energy sub level
2 = electrons

Question 22

what are the maximum amount of electrons for each energy sub level?

Answer 22

s = 2
p = 6
d = 10
f = 14

Question 23

________ electrons occupy the orbitals of the lowest energy first. 3d is ______ than 4s, but 4s is ______ than 3d

________ an orbital can have at most 2 electrons; to occupy the same orbital, two electrons must have opposite spins

________ elections occupy the energy in a way that makes the number of electrons with the same spin as large as possible

Answer 23

Aufbau principle, higher in energy, farther away from the nucleus

Pauli exclusion principle

Hund’s rule

Question 24

D level =
look at notes and periodic table to see how sub levels are separated

Answer 24

n-1
reference

Question 25

noble gas configuration noble gas _______ an element __________ are the same as noble gases

Answer 25

above ion configurations

Question 26

________ energy level is taken away first. ex 4s is taken away and then 3d

Answer 26

outer

Question 27

______ influence the stability of an atom

Answer 27

neutrons

Question 28

elements with similar chemical and physical properties are placed together within _________

Answer 28

groups

Question 29

metals are in groups ___________ some in 13-15. group 1: group 2: group 3-12:

Answer 29

1-12 alkali metals alkali earth metals transition metals

Question 30

What are the properties of metals?

Answer 30

high melting points solid at room temperature very reactive conductive shiny malleable and ductile good conductor of heat

Question 31

nonmetals are located in the _____________ they tend to _________ valence electrons ______ do not react

Answer 31

upper right gain noble gases

Question 32

What are the properties of nonmetals?

Answer 32

stable not reactive low melting points more likely to be gases at room temp brittle poor conductivity dull

Question 33

______ hold valence electrons tightly

Answer 33

nonmetals

Question 34

What are the properties of metalloids

Answer 34

solid at room temp semiconductor shiny brittle behaves like nonmetals

Question 35

same charge - ______ opposite charge - _______

Answer 35

repulsion attraction

Question 36

more protons = _______ force of attraction is inversely proportional to distance going down a column; energy levels increase so distance increases

Answer 36

more force

Question 37

the attractive force of a nucleus is __________________. Each electron gets the ______ attractive force of the nucleus

Answer 37

not divided among the electrons in an atom full

Question 38

groups increase the ________ periods increase the ________

Answer 38

distance, protons

Question 39

________ will always overweigh ________. ----- is a bigger factor

Answer 39

distance, protons

Question 40

_______ the distance between an atom's nucleus _______ as you go down a group This is because as you go down the energy levels increase, therefore _____ increases ______ going across a period, because __________ When attraction is stronger, the valence electrons are closer causing radius to decrease

Answer 40

atomic radius/ionic radius increases, distance decreases, protons make it hold closer to the nucleus

Question 41

losing electrons makes ion ________ because there are less _______ ionic radius decreases for _______ and increases for ______-

Answer 41

smaller, energy levels, cations, anions

Question 42

_______ amount of energy needed to remove an electron from a natural atom. it is the opposite of electronegativity _________ as you go down a group because the attraction is weaker and it is easier to take an electron away _________ when going across because there are more protons so more attraction, therefore harder to remove an electron

Answer 42

1st ionization energy decreases increases

Question 43

________ measure of the tendency of an atom to attract a bonding pair of electrons ______ going down a group because more energy levels makes it harder to attract electrons ________ don't have this ______ going across because more protons makes it easier to attract

Answer 43

electronegativity decreases noble gases increases

Question 44

_______ ability to lose an election during a chemical reaction due to _______ energy ______ across the periods because it gets farther away from the metals ________ going down from top to bottom

Answer 44

metallic character, low ionization energy decreases increases

Question 45

________ means that you have already removed the valence electrons and are attacking core electrons

Answer 45

big jump