mod 1 ch 1

Question 1

label

Answer 1

A: Mass number (protons + neutrons)
X: Element symbol (one or two letters)
Z: atomic number (number of protons)

Question 2

what is this

Answer 2

the atomic mass, weighted average mass in amu (atomic mass units) of an elements isotope

Question 3

define isotopes

Answer 3

atoms with the same atomic number but different mass numbers

Question 4

what is the solution to the wave equation

Answer 4

wave function or orbital

Question 5

what are the four different kinds of orbitals

Answer 5

s, p, d, f

Question 6

what are the three configurations a p orbital can have

Answer 6

Question 7

each orbital can have up to two electrons that must have ___________ _______.

Answer 7

opposite spins

Question 8

label

Answer 8

2 - s orbital (2)
8 - s and p orbitals (2 + 6)
18 - s, p, and d orbitals (2 + 6 + 10)

Question 9

as electron shells get farther from the nucleus

Answer 9

they get bigger and increase in energy

Question 10

when filling orbitals, electrons must fill up the same energy orbital before…

Answer 10

pairing up with an electron of opposite spin

Question 11

valence shell

Answer 11

outermost shell occupied by electrons

Question 12

valence electrons

Answer 12

electrons in the outermost shell (valence shell)

Question 13

what is chemical bonding theory

Answer 13

atoms form bonds because the resulting compound is more stable than the separate atoms

Question 14

ionic bonds

Answer 14

formed as the result of electron transfers, ions formed held together by an electrostatic attraction

Question 15

label the product

Answer 15

IONIC COMPOUND

Question 16

label the product

Answer 16

COVALENT COMPOUND

Question 17

covalent bond

Answer 17

formed by sharing of electrons between nonmetals

Question 18

It is energetically favorable for non-metallic elements to ________ ________ in order to achieve electron configuration of nearest inert gas

Answer 18

SHARE ELECTRONS

Question 19

how many covalent bonds does hydrogen form

Answer 19

one

Question 20

how many covalent bonds does carbon form

Answer 20

four

Question 21

how many covalent bonds does oxygen form

Answer 21

two

Question 22

how many covalent bonds does nitrogen form

Answer 22

three

Question 23

what does the valence bond theory state

Answer 23

covalent bonds form when two atoms approach each other closely so that an orbital containing 1e- overlaps with another orbital containing 1e-

Question 24

what is bond length

Answer 24

ideal distance between nuclei that leads to maximum stability

Question 25

when a bond breaks, energy is

Answer 25

absorbed

Question 26

when a bond is formed, energy is

Answer 26

released

Question 27

what are the hybridizations strongest to weakest

Answer 27

sp - strongest sp2 - middle sp3 - weakest

Question 28

if an atom only has sigma bonds its hybridization is

Answer 28

sp3

Question 29

if an atom has one double bond and two single bonds its hybridization is

Answer 29

sp2

Question 30

if an atom has one triple bond and a single its hybridization is

Answer 30

sp

Question 31

what are the hybridizations bond lengths from longest to shortest

Answer 31

sp3 - longest bond length sp2 - middle sp - shortest bond length

Question 32

what is the molecular geometry of an sp2 hybridized atom and what is its bond angle

Answer 32

trigonal planar, 120

Question 33

what is the molecular geometry of an sp3 hybridized atom and what is its bond angle

Answer 33

tetrahedral, 109.5

Question 34

what is the molecular geometry of an sp hybridized atom and what is its bond angle

Answer 34

linear,180

Question 35

what is the Formal Charge formula

Answer 35

FC = valence electrons - lines - dots

Question 36

what are the three ways oxygen exists

Answer 36

Question 37

what are the three ways carbon exists

Answer 37

Question 38

what are the three ways nitrogen exists

Answer 38

Question 39

in resonance if an atom must have a charge but the negative charge on the most ____________ atom

Answer 39

electronegative

Question 40

what are the three types of resonances

Answer 40

type I - when a molecule has a positive charge adjacent to a double/triple bond type II - when a molecule has a negative charge or a lone e- pair adjacent to a double or triple bond type III - when the molecule has BOTH a positive and negative charge adjacent to each other OR if the molecule has no charge but at least one double or triple bond

Question 41

what are the steps for type I resonance?

Answer 41

1. start with the positive charge and label it #1. count through three consecutive atoms making sure there is a double or triple bond between atoms #2 and #3 2. break the double/triple bond between atoms #2 and #3 and put it between atoms #1 and #2. place the positive charge on atom #3

Question 42

what are the steps for type II resonance?

Answer 42

1. start with the positive charge and label it #1. count through three consecutive atoms making sure there is a double or triple bond between atoms #2 and #3 2. lone pair/negative charge on atom #1 makes a double bond between atoms #1 and #2. the double/triple bond between atom #2 and #3 breaks and leave a lone pair on atom #3.

Question 43

what are the steps for type III resonance?

Answer 43

1. if a molecule has no charge but it has a double or triple bond: break the double/triple bond between atoms #1 and #2. place a lone pair and a negative charge on atom #1 and a positive charge on atom #2 2. if the molecule has both a positive and negative charge adjacent: move the lone pair from atom #1 and make a double bond between atoms #1 and #2