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Chemistry > Test 3 > Flashcards

Test 3 Flashcards

1
Q

4th quantum spin(s)

A

Electron is a spinning charge, can either spin up or down. Represented by either +1/2 or -1/2

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2
Q

Auf bau principal

A

lowest energy occupied first

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3
Q

Polyexclusion principal

A

each electron has a unique set of quantum numbers

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4
Q

Hund’s principal

A

parallel spins in different boxes before pairing up to minimize C-e repulsion

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5
Q

Magnetic properties

A

-related to unpaired electrons

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6
Q

Diamagnetic

A

Unaffected by magnetic field, all electrons paired

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7
Q

Paramagnetic

A

Attracted by magnetic field, has unpaired electrons

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8
Q

Electron configuration of Ions

A

Cations loose e
Highest n always looses first
If more than one highest n highest l lost first

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9
Q

Electron configuration of Anions

A

gain e to get to noble gas configuration

add e as usual

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10
Q

Valence electrons

A

part of s and p orbitals and non filled f and d orbitals

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11
Q

non valence electrons

A

filled d and f orbitals are not valence electrons

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12
Q

Electron configuration of Cr

A

[Ar}4s^13d^5

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13
Q

Electron configuration of Cu

A

[Ar] 4s^13d^10

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14
Q

Effective nuclear charge

A

“charge” felt by other electrons. Ability to pull in electrons

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15
Q

How to calculate Zeff

A

Z(# of protons) - S(screening electrons closer to the nucleus)

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16
Q

Periodic table ->(Zeff)

A

Zeff increases as #of protons increases, but not the # of screening electrons

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17
Q

Periodic Table goes down(Zeff)

A

Zeff is constant

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18
Q

Periodic trends in atomic size

A

n and Zeff
As n increases, radius increases (PT goes down)
As Zeff increases, radius decreases (PT ->)

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19
Q

Size of transition elements

A

their sizes do not change much

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20
Q

Size of atoms vs cations

A

Cations(+) < atoms

Because Zeff increases

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21
Q

Size of atoms vs anions

A

Anions(-) > atoms

Because Zeff decreases

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22
Q

Trends in first ionization energies

A

closer is harder to ionize and vice versa. As Zeff increases leads to harder removal. As n increases, becomes easier to remove.

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23
Q

2nd and higher ionization energie

A

I1 < I2 < I3 < …

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24
Q

Ionic bonding

A

A cation and an Anion

electrons are given

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25
Q

Covalent bond

A

Generally non-metal + non-metal

electron sharing

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26
Q

Metallic bonding

A

electrons are mobile in what is called an “electron sea”

conductors

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27
Q

Why do covalent bonds share electrons

A

To get lower in energy

28
Q

Lattice energy

A

the energy it takes to separate one mol of ionic into infinite separation

29
Q

Coulomb’s law equation

A

E = (kQ1Q2)/R

30
Q

Electronegativity

A

The force that an atom attracts electrons in a covalent bond.

31
Q

As # of bonds increase

A

strength of the bond does too

32
Q

Formal charge

A

Charge on an atom in a molecule by assigning one e- to each end of a single bond. Can be calculated by using original # of electrons - current #

33
Q

Sum of the formal charges

A

charge on species. represents the charge of the molecule. Wants each formal charge to be as small as possible

34
Q

Electron poor

A

When an atom is lacking an electron to achieve octet rule, but maintains 0 formal charge

35
Q

electron rich

A

an atom has too many valence electrons, but still maintains 0 formal charge

36
Q

odd electron

A

an atom has an unpaired valence electron, but still maintains 0 formal charge

37
Q

Bond energy

A

it takes energy to break a bond and releases energy when a bond is formed. The average value can be found on the table at the back of the data sheet

38
Q

molecular geometry

A

shapes of molecules and bond angles. It takes at least 3 atoms to make an angle

39
Q

steric number (sn)

A

number of electron groups around an atom. Lone pairs + atoms attached to central atom

40
Q

example of electron poor molecule

A

BF3

41
Q

example of odd electron

A

NO

42
Q

example of electron rich

A

PF5

43
Q

Angle and name of steric number 2

A

180 and linear

44
Q

angle and name of sn 3

A

120 degrees and trigonal pyramid

45
Q

name and angle of sn 4

A

109 degrees and tetrahedral

46
Q

name and angle of sn 5

A

6 90 degrees, 2 120 degrees and 1 180 degrees, trigonal bypyramid

47
Q

angle and name of sn 6

A

90 and 180 degrees, octahedral/square pyramidal

48
Q

dipole moment and polarity

A

if a force of attraction from a polar bond creates a net vector that is not 0, the molecule is polar

49
Q

Anion

A

negatively charged ion

50
Q

cation

A

positively charge ion

51
Q

Orbital hybridization

A

When orbitals intersect during bonding

52
Q

Types of hybridization

A 
SN 2: sp, p+p
SN 3: sp2, p
Sn 4: sp3
SN5: sp3d
SN6: sp3d2
53
Q

Single bond type of hybridization

A

Sigma

54
Q

Double bond type of hybridization

A

pi

55
Q

Triple bond type of hybridization

A

sigma and pi

56
Q

Intermolecular forces

A

forces between molecules

57
Q

Dipole dipole interaction

A

Polar molecules, the more polar it is, the higher the dipole-dipole force

58
Q

London dispersion force

A

Depends on the number of electrons

the higher the molar mass, the higher the force

59
Q

Hydrogen bonding

A

If H is connected to a small electro negative element(F,O,N), it is attracted to a lone pair on another electro negative element

60
Q

Strength of each inter molecular forces

A

Hydrogen bonding > dipole - dipole > london dispersion force

61
Q

boiling point related to inter molecular forces

A

The higher the inter molecular forces, the higher the boiling point

62
Q

Isomer

A

Two molecules with the same molecular formula but different structures(Ie Ch3OCH3 and CH3CH2OH)

63
Q

vapor pressure in relation to molar mass

A

the smaller the molar mass the higher the vapor pressure

64
Q

vapor pressure compared to intermolecular forces

A

higher the forces, lower the vapor pressure

65
Q

Vapor pressure in relation to temperature

A

vp increases as t increases

Chemistry (5 decks)

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