Bonding

Question 1

intramolecular bonding

Answer 1

looking in at a molecule

Question 2

ionic bonding

Answer 2

the complete transfer of 1 or more electrons from 1 atom to another

Question 3

why do atoms bond

Answer 3

to reach an arrangement whereby there is 8 electrons in the outermost shell (octet rule)

Question 4

shape of ionic compounds

Answer 4

crystal lattices

Question 5

boling point of ionic compounds
high or low

Answer 5

high

Question 6

melting point of ionic compounds
high or low

Answer 6

high

Question 7

ionic compounds at room temperature
solid or liquid (usually)

Answer 7

solid

Question 8

do ionic compounds conduct electricity

Answer 8

no unless in a molten or dissolved state

Question 9

do covalent compounds conduct electricity

Answer 9

no as there are no ions

Question 10

covalent bonding

Answer 10

Sharing of electrons

Question 11

7 diatomic molecules

Answer 11

H2
O2
N2
CL2
BR2
I2
F2

Question 12

diatomic molecules are

Answer 12

2 atoms of the same element bonding together

Question 13

diatomic molecules are polar or non polar

Answer 13

non polar

Question 14

Sigma bonding

Answer 14

all single covalent bonds
head on overlap or atomic orbitals

Question 15

Pi bonding

Answer 15

sideways overlap or atomic orbitals

Question 16

sigma or pi: compound with a double bond

Answer 16

1 sigma 1 pi

Question 17

sigma or pi: compound with a triple bond

Answer 17

1 sigma 2 pi

Question 18

sideways overlap or atomic orbitals

Answer 18

pi bonding

Question 19

head on overlap or atomic orbitals

Answer 19

sigma bonding

Question 20

5 shapes of covalent compounds

Answer 20

Linear
Triangular planar
Tetrahedral
Pyramidal
V-shaped

Question 21

bond angle of linear compound

Answer 21

180

Question 22

bond angle of triangular planar compound

Answer 22

120

Question 23

bond angle of v shaped compound

Answer 23

104.5

Question 24

bond angle of tetrahedral compound

Answer 24

109.5

Question 25

bond angle of pyramidal compound

Answer 25

107

Question 26

VSEPR theory

Answer 26

Valence shell electron pair repulsion

Question 27

what is the VSEPR theory

Answer 27

lone pair/lone pair > lone pair/bond pair>bond pair/bond pair > = ' cause greater repulsion than'

Question 28

electronegativity

Answer 28

the relative attraction that an atom in a molecule has for the shared pair of electrons in a covalent bond

Question 29

the slight positive goes to the

Answer 29

lower number

Question 30

the slight negative goes to the

Answer 30

higher number

Question 31

what has more affect on if a molecule is polar or non polar shape or electronegativity

Answer 31

shape

Question 32

A polar molecule is

Answer 32

One where there is distance between the partial positive values and partial negative charges

Question 33

A non-polar molecule is

Answer 33

One in which the centre of partial positive charges coincides with the centre of partial negative charges and they cancel each other out

Question 34

if the electronegativity value is > 1.7

Answer 34

ionic

Question 35

if the electronegativity value is < or equal to 1.7

Answer 35

covalent

Question 36

intermolecular bonding

Answer 36

bonding between molecules

Question 37

3 types of intermolecular bonds

Answer 37

van der waal forces dipole-dipole forces hydrogen bonding

Question 38

van der wal forces x4

Answer 38

weak temporary exist between non polar molecules, diatomic molecules and noble gases low boiling points

Question 39

dipole-dipole x3

Answer 39

permanent stronger than van der waal forces but not stronger than hydrogen bonds or covalent bonds found in most polar substances unless it is a hydrogen bond

Question 40

hydrogen bonds x4

Answer 40

only to oxygen nitrogen or fluorine strong give rise to high boiling points extremely useful e.g. kevlar (a material used for fire retardant clothing and bullet proof vests) water surface tension