Bonding

Question 1

cation

Answer 1

positively charged ion

Question 2

anion

Answer 2

negatively charged ion

Question 3

dative bond

Answer 3

a covalent bond where both electrons in the shared pair are donated from the same atom

Question 4

Covalent bond

Answer 4

the electrostatic attraction between nuclei of two non metal atoms and the bonding electrons of their outer shells. no electrons are transferred, they are only shared

Question 5

shorter bond length means

Answer 5

greater bond strength as bonding pair is closer to atoms nucleus

Question 6

as number of shared electrons increases, bond length

Answer 6

decreases

Question 7

linear bond angle

Answer 7

180

Question 8

trigonal planar bond angle

Answer 8

120

Question 9

tetrahedral bond angle

Answer 9

109.5

Question 10

trigonal bipyramidal bond angle

Answer 10

90 and 120

Question 11

octahedral bond angle

Answer 11

90

Question 12

how many degrees is subtracted when a bond pair is replaced with a lone pair eg: trigonal planar to bent

Answer 12

-2

Question 13

valence shell electron pair repulsion theory

Answer 13

All pairs of valence electrons will repel each other to the maximum separation that they can where they experience the minimum amount of repulsion.

Question 14

pyramidal bond angle

Answer 14

107

Question 15

bent bond angle

Answer 15

118 or 104.5

Question 16

do bond pairs or lone pairs repel more

Answer 16

lone pairs

Question 17

electronegativity

Answer 17

Measures the attraction of a bonded atom for the pair of electrons in a covalent bond

Question 18

3 most electronegative elements

Answer 18

Fluorine, oxygen and nitrogen

Question 19

dipole

Answer 19

an area of slight positive or negative charge

Question 20

what leads to a polar covalent bond

Answer 20

electronegativity difference

Question 21

where does an electron lie in a polar covalent bond and what does this cause

Answer 21

closer to the more electronegative atom, giving the more electronegative atom a slight negative charge and the less electronegative atom a slight positive charge

Question 22

polar molecule

Answer 22

a molecule which can be split into 2 overall dipoles

Question 23

can symmetrical molecules be polar, why

Answer 23

no because the dipoles for each end cancel out

Question 24

dipole-dipole interactions

Answer 24

both molecules have permanent dipoles which cause them to attract eachother

Question 25

dipole-induced dipole interactions

Answer 25

permanent dipole induces a dipole on another molecule which causes them to attract

Question 26

london forces

Answer 26

instantaneous dipoles form due to electron movement causing momentary attraction

Question 27

what happens to london forces as the size of a molecule increases, why

Answer 27

the strength of london forces increases as there are more electrons to form a stronger instantaneous dipole

Question 28

order of intermolecular forces in increasing strength

Answer 28

london forces —–> dipole-dipole —–> hydrogen bonds

Question 29

where does hydrogen bonding occur

Answer 29

between molecules that have a F, O or N that has a lone pair of electrons and is also covalentally bonded to a H atom

Question 30

what is a hydrogen bond

Answer 30

an extra strong dipole-dipole interaction

Question 31

why is water denser than ice

Answer 31

hydrogen bonds in water holds molecules closer together than the lattice it forms when frozen