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chem 227 > mod 1 ch 1 > Flashcards

mod 1 ch 1 Flashcards

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1
Q

label

A

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

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2
Q

what is this

A

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

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3
Q

define isotopes

A

atoms with the same atomic number but different mass numbers

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4
Q

what is the solution to the wave equation

A

wave function or orbital

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5
Q

what are the four different kinds of orbitals

A

s, p, d, f

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6
Q

what are the three configurations a p orbital can have

A
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7
Q

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

A

opposite spins

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8
Q

label

A

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

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9
Q

as electron shells get farther from the nucleus

A

they get bigger and increase in energy

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10
Q

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

A

pairing up with an electron of opposite spin

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11
Q

valence shell

A

outermost shell occupied by electrons

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12
Q

valence electrons

A

electrons in the outermost shell (valence shell)

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13
Q

what is chemical bonding theory

A

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

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14
Q

ionic bonds

A

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

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15
Q

label the product

A

IONIC COMPOUND

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16
Q

label the product

A

COVALENT COMPOUND

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17
Q

covalent bond

A

formed by sharing of electrons between nonmetals

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18
Q

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

A

SHARE ELECTRONS

19
Q

how many covalent bonds does hydrogen form

A

one

20
Q

how many covalent bonds does carbon form

A

four

21
Q

how many covalent bonds does oxygen form

A

two

22
Q

how many covalent bonds does nitrogen form

A

three

23
Q

what does the valence bond theory state

A

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

24
Q

what is bond length

A

ideal distance between nuclei that leads to maximum stability

25
Q

when a bond breaks, energy is

A

absorbed

26
Q

when a bond is formed, energy is

A

released

27
Q

what are the hybridizations strongest to weakest

A

sp - strongest
sp2 - middle
sp3 - weakest

28
Q

if an atom only has sigma bonds its hybridization is

A

sp3

29
Q

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

A

sp2

30
Q

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

A

sp

31
Q

what are the hybridizations bond lengths from longest to shortest

A

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

32
Q

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

A

trigonal planar, 120

33
Q

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

A

tetrahedral, 109.5

34
Q

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

A

linear,180

35
Q

what is the Formal Charge formula

A

FC = valence electrons - lines - dots

36
Q

what are the three ways oxygen exists

A
37
Q

what are the three ways carbon exists

A
38
Q

what are the three ways nitrogen exists

A
39
Q

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

A

electronegative

40
Q

what are the three types of resonances

A

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

41
Q

what are the steps for type I resonance?

A
  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
42
Q

what are the steps for type II resonance?

A
  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.
43
Q

what are the steps for type III resonance?

A
  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

chem 227 (10 decks)

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