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A-level Chemistry > Chapter 5 Electrons and Bonding > Flashcards

Chapter 5 Electrons and Bonding Flashcards

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1
Q

what properties do electrons have

A

electrons have the properties of both a particle and a wave

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2
Q

what are the four sub shells represent the principle quantum shells

A

s sub shells
p sub shells
d sub shells
f sub shells

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3
Q

what happens to electrons closer to the nucleus

A

they are lower in energy because the charges of the electron and proton cancel

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4
Q

what are the ‘s’ sub shells shape

A

spheres

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5
Q

what are the ‘p’,’d’,’f’ sub shells shape

A

dumbells in the x,y and z axis

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6
Q

why do electrons go around in pairs

A

electrons go round in pairs because they spin either clockwise or anticlockwise and pair up to cancel out spins

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7
Q

what is the first electron configuration rule

A

> orbitals fill with electrons in a specific order to produce the lowest energy state possible

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8
Q

what is the second electron configuration rule

A

> orbitals fill in order of increasing energy

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9
Q

what is the third electron configuration rule

A

> where there is more than one orbital with the same energy they fill simply at first and electrons have parallel spins

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10
Q

what is the fourth electron configuration rule

A

when every orbital of the same energy is singly occupied the electrons then start to pair up with opposite spins

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11
Q

what does the large number for electron configuration represent

A

the principle quantum shell

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12
Q

what does the letter for electron configuration represent

A

the sub shell

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13
Q

what does the number in the super script for electron configuration represent

A

number of electrons in the sub shell

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14
Q

what is the max number of electrons in the ‘s’ sub shell

A

2

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15
Q

what is the max number of electrons in the ‘p’ sub shell

A

6

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16
Q

what is the max number of electrons in the ‘d’ sub shell

A

10

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17
Q

what is the max number of electrons in the ‘f’ sub shell

A

14

18
Q

what is the max number of electrons per orbital

A

2

19
Q

how do you write the short hand electron configuration

A

[Previous Noble Gas] outer shell orbitals

20
Q

what does the position of the element in the periodic table correspond to

A

the highest energy sub shell being filled

21
Q

what is the transitional metal ion electron configuration rule

A

when shells are filling 4s fills before 3d because it is lower in energy. 4s empties first because it is further away from the nucleus

22
Q

what is an orbital

A

region around the nucleus that can hold a maximum of 2 electrons

23
Q

what is ionic bonding

A

bonding between a metal and a non-metal caused by electrostatic attraction between oppositely charged ions which arises when electrons are transferred

24
Q

what 2 things happen to metals in ionic bonding

A

they lose outer shell electrons

form positively charged cations

25
Q

what 2 things happen to non metals in ionic bonding

A

they gain outer shell electrons

form negatively charged anions

26
Q

how is a giant ionic lattice formed

A

when each ion attracts many others of the opposite charge

27
Q

what does the giant ionic lattice structure cause the ion to be

A

strong and crystalline

28
Q

why ionic compounds have high melting and boiling points

A

the electrostatic forces are very strong so need lots of energy to be broken

29
Q

why are most ionic compounds soluble in water

A

water is a polar molecule which breaks the ionic bond and forms an aqueous ion

30
Q

why can ions in solution or molten conduct electricity

A

the ions are no longer in the giant lattice structure and are free to move

31
Q

what is BIN MIX

A

BIN > Breaking Is eNdothermic

MIX > Making Is eXothermic

32
Q

what three things does the solubility of the ionic compound depend on

A

> relative strength of ionic attraction
water - water bond attraction
attraction between ions and water

33
Q

what is covalent bonding

A

involves sharing electrons as orbitals overlap between non-metals

34
Q

do covalent bonds need a full outer shell of electrons

A

no

35
Q

what is expansion of octect

A

principle quantum shells of 3 and above can have more than 8 electrons in their outer shell because they have an empty d sub shell

36
Q

what are bonding pairs

A

electron pairs that form bonds

37
Q

what are lone pairs

A

pairs of electrons not involved in bonding

38
Q

what is dative covalent bonding

A

a covalent bond where at least one pair of electrons come from the same atom

39
Q

what do more bonds mean

A

the bond gets shorter and stronger

40
Q

what is average bond enthalpy

A

the amount of energy needed to break or make a bond

A-level Chemistry (19 decks)

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