Chemical Bonding

Question 1

Ionic

Answer 1

complete transfer of 1 or more electrons from one atom to

another

Question 2

Covalent

Answer 2

some valence electrons shared between atoms

Question 3

polar covalent

Answer 3

somewhere in between ionic and covalent

Question 4

why do elements form compounds

Answer 4

to “hold” a full outer (valence shell) of electrons…….Octet rule

Question 5

Valence electrons are …… …… …….. Core e are ///

Answer 5

involved in bonding, not

Question 6

covalent bonding arises from….

Answer 6

the mutual attraction of 2 nuclei for the

same electrons

Question 7

valence electrons are in

Answer 7

the outer shell.

Question 8

Due to the bond polarity the H–Cl bond energy is…..

Answer 8

is GREATER than expected for a “pure” covalent bond

Question 9

electronegativity

Answer 9

a measure of the ability of an atom in a molecule to attract electrons to itself

Question 10

the diff between pure bond energy and real bond energy is prop to

Answer 10

electronegativity

Question 11

which bond is more polar? o—h or o—f

Answer 11

oh

Question 12

polar or..

Answer 12

dipolar

Question 13

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

Answer 13

electronegativity

Question 14

higher electro negative difference means

Answer 14

high electric field across the molecule.

Question 15

even if bonds are polar, some molecules are not polar …

Answer 15

the symmetry cancels it.

Question 16

is CO2 a polar molecules?

Answer 16

no.

Question 17

is methane polar?

Answer 17

no

Question 18

single bond

Answer 18

can rotate easily

Question 19

double bond

Answer 19

cant rotate.

Question 20

bond length

Answer 20

is the distance between nuclei of two bonded atoms

Question 21

bond order

Answer 21

the number of bonds between pairs of atoms

Question 22

bond order prop to

Answer 22

bond strength& length

Question 23

bong length depends on

Answer 23

size of bonded atoms

Question 24

bond strength

Answer 24

the energy required to break a bond

Question 25

bond strength increase as bond order

Answer 25

increases

Question 26

resonance structure the bond order is

Answer 26

non whole number

Question 27

breaking bonds

Answer 27

requires energy(endo)

Question 28

bonds formed

Answer 28

releases energy(exo)

Question 29

intramolecular

Answer 29

covalent, ionic

Question 30

intermolecular bonding

Answer 30

van der waals, hydrogen, dipole dipole

Question 31

ion dipole forces-e.g NA+ in sodium chloride molecule attracting o- in h20

Answer 31

attraction between ions and permanent dipoles

Question 32

hydrated ions

Answer 32

water can interact with + ions to give these

Question 33

dipole dipole forces

Answer 33

bind molecules that have permanent dipoles to one another

Question 34

influence of di-di forces is seen in

Answer 34

boiling points

Question 35

hydrogen bonding:

attraction between a /// pair on one ////// and a hydrogen atom attached to an ////-element on another

Answer 35

..

Question 36

h bonding is strongest with

Answer 36

O, N, F

Question 37

Why N,O, AND F?

Answer 37

they are the most electro- elements on table.

Question 38

the hydrogen bonding in water is very strong

Answer 38

there are two lone pairs of e- around o and two h on each.

Question 39

how does o2(non polar) and i2 dissolve in water

Answer 39

water INDUCES dipole in o2 etc

Question 40

polarisation

Answer 40

inducing a dipole

Question 41

polarisibilty of a molecule

Answer 41

degree to which e- cloud of a molecule can be distorted

Question 42

larger molecules

Answer 42

> larger induced dipoles»>larger boiling points

Question 43

boiling point is a ….. of the ……. of ……… forces

Answer 43

meausre, strength, intermolecular

Question 44

………forces are in non …..molecules

Answer 44

induced, polar