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Chemistry Year 12 > Module 2.2 > Flashcards

Module 2.2 Flashcards

1
Q

What is an orbital

A

a region of space where one might find up to two electrons with opposite spins

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2
Q

what is ionic bonding

A

the electrostatic attraction between position and negative ions

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3
Q

what is covalent bonding

A

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

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4
Q

what is relative atomic mass

A

the weighted mean mass of an atom of an element compared with 1/12 of the mass of carbon-12

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5
Q

what is relative isotopic mass

A

the mean mass of an atom of an isotope compared with 1/12 of the mass of carbon-12

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6
Q

what is empirical formula

A

simplest whole number ratio of atoms in a substance

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7
Q

how do you calculate number of electrons in a shell

A

2n^2

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8
Q

how do electrons enter shells

A

at the lowest energy shell available

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9
Q

whats the shape and occurrence of s orbitals

A

spherical shape, one in every principal level

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10
Q

whats the shape and occurrence of p orbital

A

dumbbell shape, 3 in levels 2 upwards

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11
Q

whats the shape and occurrence of d orbital

A

various shapes, 5 in levels 3 upwards

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12
Q

whats the shape and occurrence of f orbital

A

various shapes, 7 in levels 4 upwards

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13
Q

what energy level is lower, 4s or 3d

A

4s

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14
Q

what two elements have different electronic configuration and how

A

chromium - fills 3d singularly then one in 4s
copper - fills 3d in pairs and one in 4s

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15
Q

how do you work out the electronic configuration of ions

A

take from the highest occupied orbital (4s before 3d)

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16
Q

what is a giant ionic lattice

A

oppositely charged ions held in a regular repeating 3D lattice by electrostatic attraction

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17
Q

properties of ionic compounds

A

very brittle, insoluable in non-polar solvents (polar solvents stabilise the separated ions because the delta+ atoms attract the the negative ions and vice versa), doesnt conduct as a solid as the ions are in a fixed position in the lattice, but does molten and the ions are free to move as the lattice structure is broken

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18
Q

what are the properties of simple covalent molecules

A

never conduct (no free ions or delocalised electrons), more soluable in organic solvents rather than water, low boiling point as intermolecular forces are always weak (get strong-ER as molecules get a larger surface area)

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19
Q

what is dative or (coordinate) covalent bonding

A

a covalent bond where both of the electrons being shared come from one of the atoms

20
Q

what happens to the main atom in dative bonding

A

it becomes slightly positive as more of its negative electrons are shared

21
Q

what atoms can expand their octet

A

non metals in groups 5-7 from period 3 and onwards

22
Q

how many covalent bonds can group 5 elements form

A

3 or 5

23
Q

how many covalent bonds can group 6 elements form

A

2,4 or 6

24
Q

how many covalent bonds can group 7 elements form

A

1,3,5 or 7

25
Q

what is PFv5 called

A

phosphorus pentaflouride

26
Q

what is SFv6 called

A

sulphur hexafluoride

27
Q

what are the general properties of giant covalent structures/networks/macromolecules

A

very high melting point due to many strong covalent bonds, don’t conduct bar graphite and graphene (1 spare electron), usually hard because of rigid tetrahedral structure (diamond and silica) but graphite is soft

28
Q

name the main giant covalent structures

A

diamond, graphite, graphene silica (SiOv2)

29
Q

what is electronegativity

A

the ability of an atom to attract the bonding pair of electrons in a covalent bond

30
Q

how is electronegativity measured

A

pauling scale
increased up and right

31
Q

what’s the criteria to be a polar molecule

A

polar bond and unsymmetrical molecule

32
Q

what can we use to measure the strength of a covalent bond

A

average bond enthalpies

33
Q

when do london forces occur

A

between all atoms/molecules

34
Q

how do london forces happen

A

when electrons (always in constant motion) are momentarily more on one side of a molecule creating a temporary/instantaneous dipole which causes an induced dipole in the other molecule/atom

35
Q

when do permanent dipole-dipole interactions happen

A

between two polar molecules

36
Q

what does hydrogen bonding happen between

A

a lone pair on a F O or N atom (that’s bonded with a hydrogen) and an H atom (that’s bonded with F O or N)

37
Q

what happens to boiling point when hydrogen bonds are present

A

higher than expected because the forces are strong and takes lots of energy to overcome

38
Q

describe the structure of ice

A

each molecule hydrogen bonded to 4 others in tetrahedral structure - open lattice structure - volume is larger than liquid so less dense

39
Q

when is waters maximum density and why

A

4°C because when ice melts the structure collapses slightly and molecules come closer - then move a little further apart as the get more energy when heated

40
Q

how many lone pairs do O and N have when bonded with hydrogen

A

2

41
Q

how many lone pairs does F have when bonded with hydrogen

A

3

42
Q

why is hydrogen bonding so strong

A

because the interaction is extremely polar (only with the most electronegative elements) AND the small sizes of H F N and O are concentrated in a small volume so a high charge density

43
Q

what is a permanent dipole

A

the charge different between the two bonded atoms in a polar bond

44
Q

why are symmetrical molecules never polar molecules

A

because the dipoles act in different directions in an equal distribution so they cancel eachother out

45
Q

how does a greater electronegativity difference impact polarity

A

greater difference = greater polarity

46
Q

what factors affect electronegativity

A

nuclear charge, distance from nucleus and electron shielding

47
Q

do you remove from 4s or 3d first for ions??

A

4s

Chemistry Year 12 (7 decks)

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