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Chemistry #yeet :) > 2.2 > Flashcards

2.2 Flashcards

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1
Q

What has To exist for hydrogen bonding to happen?

A

1) hydrogen

2) a NOF

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2
Q

Oxonium ion?

A

H30+

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3
Q

What is an orbital?

A

A region in space where one is likely to find an electron, each orbital can hold up to 2 electrons

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4
Q

What are the physical bonds from weakest to strongest ?

A

Induced dipole dipole
Permanent dipole dipole
Hydrogen bonds

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5
Q

how many electrons can an f orbital show?

A

14

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6
Q

how many electrons can a d orbital show?

A

10

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7
Q

how many electrons can a p orbital show?

A

6

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8
Q

how many electrons can a s orbital show?

A

2

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9
Q

how many electrons can the 1st shell hold?

A

2

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10
Q

how many electrons can the 2nd shell hold?

A

8

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11
Q

how many electrons can the 3rd shell hold?

A

18

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12
Q

how many electrons can the fourth shell hold?

A

32

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13
Q

what is the order of energy levels, going up?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 4d, 4f…

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14
Q

what does ionic bonding involve?

A

electrons being transferred from the metal atom to the non metal atom, allowing the elements to obtain noble gas configurations.

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15
Q

what does something have to have to hydrogen bonds?

A

hydrogen and a NOF (nitrogen oxygen fluorine)

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16
Q

how does hydrogen bonding work?

A
  • h-bonds are the strongest type of IMF
  • there is a large difference in electronegativity between the hydrogen and NOF, resulting in very strong dipole-dipole interactions called a hydrogen bond between molecules.
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17
Q

define orbital.

A

a region of space in which you are likely to find an electron, it can hold up to 2 electrons with opposite spin.

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18
Q

what is the shape of an s orbital?

A

spherical

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19
Q

what is the shape of a p orbital?

A

dumbell

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20
Q

what happens to distance between principal energy levels as you get further from the nucleus?

A

get closer together

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21
Q

what are the exceptions of the electron configuration rules?

A

CHROMIUM

COPPER

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22
Q

what is electron configuration of chromium?

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5

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23
Q

what is the electron configuration of copper?

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10

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24
Q

what is the rule for configurations of first row transition metals ?

A

when becoming ions, the electrons in the 4s orbital are removed before any electrons in the 3d orbitals.
eg: Ti+: …4s1 3d2
Ti2+: … 3d2

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25
Q

what are the 3 physical bonds, from weakest to strongest?

A

1) induced dipole dipole
2) permanent dipole dipole
3) h-bonds

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26
Q

what is the structure of ionic compounds?

A

-each ion attracts oppositely charged ions from all directions, forming a giant ionic lattice

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27
Q

why do ionic substances have a high melting and boiling point?

A

there are strong electrostatic forces between the positively and negatively charged ions. Therefore lots of heat energy is needed to overcome these forces.

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28
Q

are ionic substances soluble in water?

A

yeah

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29
Q

can ionic substances conduct electricity?

A

if they’re molten or aqueous.

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30
Q

are ionic substances brittle?

A

yes

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31
Q

why are ionic substances soluble in water?

A

water is a polar molecule. the partially negative oxygen atoms attract positive metal ions. partially positive hydrogen atoms attract negative non-metal atoms, causing it to dissolve.

32
Q

why are ionic substances brittle?

A

if you move a layer of ions, you get ions of the same charge next to eachother. the like charges repel eachother and the crystal breaks up.

33
Q

nitrate?

A

NO3-

34
Q

sulphate?

A

SO4 2-

35
Q

carbonate?

A

CO3 2-

36
Q

hydroxide?

A

OH-

37
Q

ammonia?

A

NH4+

38
Q

silver ion?

A

Ag+

39
Q

zinc ion?

A

Zn 2+

40
Q

why are covalent bonds very strong?

A

electrostatic forces between positively charged protons in the nucleus and the negatively charged electrons in both atoms.

41
Q

what is the effect of lone pairs on shape?

A

lone pairs cause extra repulsion, so bond angles are 2.5 degrees less as the other bonds are squeezed together.

42
Q

what is the shape called when it’s based on tetrahedral but has 1 lone pair?

A

pyramidal

43
Q

what’s the shape called when it’s based on tetrahedral but has 2 lone pairs?

A

angular or bent

44
Q

what is the electron repulsion theory?

A

the shape adopted by a simple molecule or ion is that which keeps repulsive forces to a minimum.

45
Q

what is the shape called when 1 atom is bonded to 3 others?

A

trigonal planar

46
Q

what is the shape called when 1 atom is bonded to 4 others?

A

tetrahedral

47
Q

what is the shape called when 1 atom is bonded to 6 others?

A

octahedral

48
Q

what is the bond angle of tetrahedral?

A

109.5

49
Q

what is the bond angle of octahedral?

A

90

50
Q

what is the bond angle of trigonal planar?

A

120

51
Q

why are simple covalent molecules a gas at room temperature?

A

they are small molecules so there are few IMFs between the molecules. little heat energyis required ti break the molecules apart. this means the substance as a low boiling point and is a gas at room temperature.

52
Q

what is disproportionation?

A

Oxidation and reduction of the same element.

53
Q

what is ionic bonding?

A

The electrostatic attraction between oppositely charged ions.

54
Q

what is covalent bonding?

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

55
Q

what is metallic bonding?

A

The electrostatic attraction between positively charged metal ions and the sea of delocalised electrons

56
Q

when explaining trends in melting/boiling points, always say…

A

…THEREFORE MORE/LESS ENERGY IS NEEDED TO BREAK IMFS

57
Q

when explaining shapes always say…

A

…pairs which REPEL

58
Q

READ THE FUCKIN QUESITON IN THE EXAM SKJHDASLKHDSAKFDSLAKDFSHDLFSK

A

yah

yeet

59
Q

why are alcohols soluble in water?

A

they form HYDROGEN BONDS with the water

60
Q

WHAT DO YOU HAVE TO REMEMBER ABOUT POLAR MOECULES

A

THEYRE NOT SYMMETRICALLLLL

61
Q

is nitrogen diatomic?

A

ye

62
Q

what bond is weaker sigma or pi

A

PI

P FOR PEAK

63
Q

what bond is stronger sigma or pi

A

SIGMA

S FOR STRONG

64
Q

Why is ice less dense than water ?

A

Ice has an OPEN lattice, molecules in ice held apart by h-bonds.

65
Q

What kind of lattice does KBr have ?

A

GIANT ionic

66
Q

What kind of lattice does ice have ?

A

Simple molecular

67
Q

write an ionic equation for silver nitrate forming a precipitate with iodide.

A

Ag+ + I- —> AgI

68
Q

what is the ion responsible for bleaching?

A

ClO-

69
Q

what’s a disadvantage of using chlorine in water purification?

A

chlorine compounds are carcinogenic/toxic/poisonous

70
Q

how do induced dipole dipole interactions arise?

A
  • uneven distribution of electrons
  • causes instantaneous dipole
  • causes induced dipoles in neighbouring molecules.
71
Q

always do the full definition of orbital

A

do it

72
Q

WHAT DO YOU HAVE TO REMEMBER ABOUT DRAWING H BONDS

A

THEY COME FROM THE LONE PAIRS

73
Q

when describing metallic bonding, always say…

A

DELOCALISED ELECTRONS

74
Q

WHEN USING BRADYS TO TEST FOR A SPECIFIC CO WHAT DO U DO

A

IT FORMS A ORANGE PPT. PURIFY THE PRODUCT ABD COMPARE MELTING POINT OF CRYSTALS TO KNOWN VALUES.

75
Q

HOW DO U DESCRIBE NON METAL MOLECULES

A

SIMPLE COVALENT

Chemistry #yeet :) (13 decks)

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