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LC Chemistry > Bonding 1 > Flashcards

Bonding 1 Flashcards

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1
Q

wcompound

A

substance made up of 2 or more different elements that are chemically combined eg carbon dioxide, water

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2
Q

octet rule

A

when bonding happens, atoms tend to reach an electron agreement with eight electrons in the outermost energy level. this is known as a stable outer octet.

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3
Q

valency

A

number of hydrogen atoms or any other monovalent element with which each atom of the element combines ie carbon can bond to 4 hydrogen atoms so its valency is 4

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4
Q

ionic bond

A

force of attraction between oppositely charged ions in a compound. they are always formed by the complete transfer of electrons from one atom to another. giving and receiving

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5
Q

transition metal

A

a metal that forms at least one ion with a partially filled d sublevel. it loses electrons from the 4s sublevel first

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6
Q

variable valency

A

there is a very small energy difference between the 4s and 3d sublevel so there can be movement of electrons between these sublevels which leads to ions with different charges. (ions can have more than one charge.)

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7
Q

how can you tell the charge on a transition metal?

A

by looking at its name (metals always form + ions) and the roman numerals give us the charge

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8
Q

what are the 2 elements not considered transition metals

A

scandium and zinc

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9
Q

why is scandium not considered a transition metal?

A

forms only 1 ion (Sc+3)
0 electrons in the 3d sublevel ie not partially filled
does not form coloured solution

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10
Q

why is zinc not considered a transition metal.

A

forms only 1 ion (Zn+2)
10 electrons in the 3d sublevel ie not partially filled
does not form coloured solution

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11
Q

which comes first when naming a compound

A

metal then the non metal

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12
Q

what is the name for a neg ion

A

anion

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13
Q

what is the name for a pos ion

A

cation

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14
Q

what sign is used to show an ionic bond in a diagram

A

an arrow

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15
Q

what must be shown outside of the brackets in an ionic bond diagram

A

the charge

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16
Q

what symbols are used to show electrons in ionic bonding diagrams

A

dots and crosses

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17
Q

what does a chemical formula tell us

A

how many atoms of each element there is in a compound

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18
Q

what charge do ionic compounds have?

A

neutral ie balanced

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19
Q

in what circumstances does crossing the charges on an ion not work?

A

if the numbers in the charges are the same (they cancel)
if the charges have a lowest common multiple ie 4 and 2 becomes 2 and 1

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20
Q

what are the steps in finding a chemical formula?

A
  1. what group is each element in
  2. decide what charge each ion has
  3. balance the charges by crossing the numbers
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21
Q

what is a polyatomic ion?

A

ions that have more than one atom

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22
Q

hydroxide

A

OH-

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23
Q

nitrate

A

NO3-

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24
Q

hydrogencarbonate

A

HCO3-

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25
Q

permagonate

A

MnO4-

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26
Q

carbonate

A

CO3-2

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27
Q

chromate

A

CrO4-2

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28
Q

dichromate

A

Cr2O7-2

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29
Q

sulphate

A

SO4-2

30
Q

sulphite

A

SO3-2

31
Q

thiosulphate

A

S203-2

32
Q

phosphate

A

PO4-3

33
Q

ammonium

A

NH4+

34
Q

how do you write the chemical formula of a polyatomic ion?

A

same as normal except for when you have more than one of the polyatomic ion you put brackets around it and then the amount after them

35
Q

molecule

A

a group of neutral atoms joined together and does not contain any ions.

36
Q

how are covalent bonds formed

A

between 2 non-metals sharing pairs of electrons

37
Q

why are bonds formed

A

so that atoms can have a full outer octet meaning it becomes more stable

38
Q

why are nobel gases never involved in bonding?

A

they already have a stable outer octet and are highly unlikely to forms bonds with themselves

MONOATOMIC!!!!

39
Q

what energy level do we draw in covalent bonding

A

only ever the outer energy level

40
Q

give 3 differences between ionic and covalent bonding

A

ionic:
conducts electricity when molten or in solution
high melting and boiling points
hard and brittle

covalent:
does not conduct electricity
low melting + boiling points
soft

41
Q

why do ionic substances conduct electricity when molten or in solution

A

for a substance to conduct electricity charge has to be able to move.
when ionic substances are solid the ions are trapped in a 3D crystal lattice and are unable to move
when ions become molten or are dispersed in solution, they become free to move and are able to conduct electricity

42
Q

what are lone pairs

A

a pair of electrons not involved in bonding

43
Q

how many of each sigma and pi is there in a single bond

A

1 sigma

44
Q

how many of each sigma and pi is there in a double bond

A

1 sigma 1 pi

45
Q

how many of each sigma and pi is there in a triple bond

A

1 sigma 2 pi

46
Q

what are the 2 types of covalent bond

A

sigma and pi

47
Q

sigma bond

A

formed by the head on overlap of atomic orbitala

48
Q

pi bonding

A

formed by the sideways overlap of p,d and f orbitals

49
Q

what happens when double bonds form?

A

first a head on overlap of 2 p orbitals (sigma)
then a sideways overlap of 2 p orbitals (pi)

50
Q

give 4 differences between a sigma and a pi bond

A

sigma:
formed first
formed by head on overlap of orbitals
involves all orbitals
more overlap of orbitals(area)
pi:
formed after a sigma bond
formed by the sideways overlap of orbitals
does not involve s orbitals
less overlap of orbitals

51
Q

what does VSEPR stand for

A

valence
shell
electron
pair
repulsion

52
Q

what is always the start of our answer for “explain/account for the shape”

A

LP/LP > LP/BP >BP/BP
<———————–
repulsion

53
Q

linear

A

180
2 bond pairs
AB

54
Q

trigonal planar

A

120
3 bond pairs
AB3

55
Q

tetrahedral

A

109.5
4 bond pairs
AB4

56
Q

pyramidal

A

107
1 lone pair, 3 bond pairs
AB3

57
Q

v-shaped

A

104.5
2 lone pair 2 bond pairs
AB2

58
Q

what forms an ionic bond

A

a metal and non metal

59
Q

why do atoms bond?

A

so they can get a stable outer octet

60
Q

when do ionic bonds form

A

when one atom (the metal) donates an e- and another accepts it

61
Q

what determines the charge on an ion

A

the no of e- it has lost or gained

62
Q

why is the boiling point of ionic compounds so high

A

an ionic compound contains a cation and an anion which are held together by a strong electrostatic force
the ions are arranged in a 3D crystal lattice the unit cell repeating in all directions
ie it takes a lot more energy to overcome these bonds

63
Q

in what way are ionic molecules arranged

A

the ions are arranged in a 3D crystal lattice the unit cell repeating in all directions for example in NaCl each Na+ ion is surrounded by 6 Cl- ions

64
Q

where are transition metals found

A

d block

65
Q

what are the properties of transition metals

A

`they form highly coloured solutions
frequently used as catalysts

66
Q

what does inert mean

A

doesn’t form bonds/react

67
Q

why are lone pairs important

A

determining the shape of a molecule

68
Q

what do you need to mention when talking about an atom gaining/loosing e- in an ionic bond?

A

which sublevel the e- is going to/from

69
Q

from what sublevel do transition metals loose e- from first?

A

4s

70
Q

what charge do ionic compounds have

A

neutral

71
Q

what do we say when explaining shape

A

lp/lp>lp/bp>bp/bp
<———————–
repulsion

state how many lp and bp are on the central atom and explain based on repulsion theory

LC Chemistry (22 decks)

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