bonding

Question 1

ionic bonding

Answer 1

oppositely charged ions attract through electrostatic forces to form a giant ionic lattice

Question 2

sulfate formula

Answer 2

SO4 2-

Question 3

hydroxide formula

Answer 3

OH-

Question 4

nitrate formula

Answer 4

NO3 -

Question 5

carbonate formula

Answer 5

CO3 2-

Question 6

ammonium formula

Answer 6

NH4 +

Question 7

single covalent bond

Answer 7

shared pair of electrons between two outer shells in order to achieve full outer shell

Question 8

multiple covalent bond

Answer 8

multiple pairs of electrons shared

Question 9

co-ordinate (dative covalent) bond

Answer 9

shared pair of electrons with both electrons supplied by one atom

Question 10

how to represent covalent or coordinate bond

Answer 10

covelant using a line
coordinate using an arrow from the lone electron pair

Question 11

metallic bonding

Answer 11

strong electrostatic force of attraction between delocalised electrons and positive ions arranged in a lattice

Question 12

four types of crystal structure

Answer 12

ionic
metallic
macromolecular
simple molecular

Question 13

crystal structure of diamond

Answer 13

macromoleular

Question 14

crystal structure of graphite

Answer 14

macromolecular

Question 15

crystal structure of ice

Answer 15

simple molecular

Question 16

crystal structure of iodine

Answer 16

simple molecular

Question 17

crystal structure of magnesium

Answer 17

metallic

Question 18

crystal structure of sodium chloride

Answer 18

ionic

Question 19

MP of macromolecular structures

Answer 19

very high mp as multiple covalent bonds to overcome which are very strong

Question 20

MP and conductivity of simple molecular

Answer 20

usually low mp due to IDD but depends if PDD or hydrogen bonding
very poor conductors as no charged particles

Question 21

MP and conductivity of ionic strucutres

Answer 21

high MP as strong electrostatic forces
conducs electricity in molten or solution as ions seperate so free to move and carry a flow of charge

Question 22

MP and conductivity of metallic substances

Answer 22

high mp due to strong electrostatic forces of attraction
high melting poins nealry alwasys solid at room temp

Question 23

explain the energy changes associated with changes of state

Answer 23

as temp rises kinetic energy of the particle increases

Question 24

bonding pairs and lone pairs of electrons are

Answer 24

charge clouds that repel each other

Question 25

arrangement of pairs of electrons in outershell of atom

Answer 25

arrange themselves as far apart as possible to minimise repulsion

Question 26

lone pair, bond pair replusion comparison

Answer 26

lone pair-lone pair repulsion> lone pair- bond pair> bond pair-bond pair

Question 27

effects of electron pair replusion on bond angles

Answer 27

lone pair- lone pair replusion reduced the bond angle

Question 28

bonding pairs , lone pairs , bond angle of linear

Answer 28

2 0 180

Question 29

bonding pairs , lone pairs , bond angle of trigonal planar

Answer 29

3 0 120

Question 30

bonding pairs , lone pairs , bond angle of tetrahedral

Answer 30

4 0 109.5

Question 31

bonding pairs , lone pairs , bond angle of trigonal biprymidal

Answer 31

5 0 120 and 90

Question 32

bonding pairs , lone pairs , bond angle of octahedral

Answer 32

6 0 90

Question 33

bonding pairs , lone pairs , bond angle of v-shape

Answer 33

2 1 117.5 and 2 2 104.5

Question 34

bonding pairs , lone pairs , bond angle of see-saw

Answer 34

4 1 119 and 89

Question 35

bonding pairs , lone pairs , bond angle of square pyramidal

Answer 35

5 1 89

Question 36

bonding pairs , lone pairs , bond angle of triangular pyramid

Answer 36

3 1 107

Question 37

bonding pairs , lone pairs , bond angle of t-shape

Answer 37

3 2 89

Question 38

bonding pairs , lone pairs , bond angle of square planar

Answer 38

4 2 90

Question 39

electronegativity

Answer 39

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

Question 40

trend in electronegativity down a group and across a period

Answer 40

decreases down a group as shielding increases increases across a period as atomic radius decreases

Question 41

causes of permentant dipole

Answer 41

electron distribution in a covalent bond between elements with different electronegativities will be unsymmetrical which produces a polar covalent bond and may cause molecule to have permentant diploe

Question 42

explain why some molecules with polar bonds do not hvae a permentant dipole

Answer 42

non-polar molecule may still contain polar bonds and the presence of symmetrical bonds in a molecules means that the delta charges cancel each other out so no permentant diople formed

Question 43

3 main types of intermoleuclar forces

Answer 43

induced dipole dipole permeant diploe dipoles hydrogen bonding

Question 44

how are melting and boiling points of simple molecular substances influenced by the strenth of these intermolecular forces

Answer 44

IDD- weakest type of intermolecular force, larger the mr the stronger the intermolecular force higher the melting point (generally lower mp though) PDD- stronger intermolecular forces than IDD weaker than hydrogen bonding of similar sized molecules, mid melting and boiling point Hydrogen bonding- much higher melting and boiling points compared to similar sized molecules without hydrogen bonding

Question 45

how does hydrogen bonding arise

Answer 45

forms between hydrogen and the 3 most electronegative atoms(nitrogen, oxegon and flourine). the lone pair on NOF attracted to the delta positive on hydrogen (shown with a dotted line)

Question 46

importance of hydrogen bonding in the low density of ice and anomalous boiling points of compounds

Answer 46

low densisty of ice- water molecules become arranged into 3D networks where each water molecule is connected to 4 other water molecules by hydrogen bonds so the water molecules in solid ice are further apart than the molecules in liquid water anomalous boiling point- requires more energy to break its hydrogen bonds before it can begin to boil