BONDING

Question 1

Ionic bonidng occurs betwen which types of elements?

Answer 1

metals and non-metals

Question 2

what type of elements loses electrons

Answer 2

metals

Question 3

what type of elements gains electrons

Answer 3

non- metals

Question 4

describe:
ionic bonding
structure
Physical properties

Answer 4

giant ionic lattice
strong ionic bonding
high melting and boiling points strong electrostatic forces of attraction between oppositely charged ions
Don’t conduct electricity as solid as ions are fixed positions
conduct electricity as liquids as ions are free to move

Question 5

describe
metallic bonding
structure
properties

Answer 5

metallic bonding
giant metallic lattice
high melting point as strong electrostatic forces of attraction between + ions and delocalised e- require lots of energy to overcome

Question 6

Macro molecular structure

Answer 6

covalent bond between atoms
macromolecular bonding
high melting and boiling point as strong covalent bond between atoms the structure requires a lot of energy to overcome
don’t conduct electricity except graphite
Diamond: no moving charges
graphite: delocalised e- layers can slide over each other

Question 7

simple molecular structure

Answer 7

strong covalent bond between atoms
weak intermolecular forces between molecules
low melting and boiling point as intermolecular forces between the molecules are weak
don’t conduct electricity as molecules are neutral so there are no moving charges electrons are localised in the bonds

Question 8

comparing metal atoms between x and y model answer

Answer 8

x has a greater charge of ….+
x has twice as many electrons in the sea of delocalised e-
x ions are smaller , meaning there is a greater density
therefore the attraction between x ions and delocalised e- is stronger

Question 9

importance of hydrogen boning

Answer 9

Ice: less dense then water because hydrogen bonds in ice hold the molecule further apart

Question 10

how does induced dipole diple arise

Answer 10

random movement of e- in one molecule leads an uneven distribution of e- , creating a temporary dipole in one molecule. This induces a dipole in the other molecule. dipoles attract

Question 11

how does permanent dipole dipole forces arrise?

Answer 11

difference in electronegativity leads to bond polarity
dipole don’t cancel therefor the molecule has an overall permanent dipole
there is an attraction between delta positive on one molecule and delta negative on an other

Question 12

how does hydrogen bonding arrise

Answer 12

large difference in electronegativity between NOF and hydrogen
creates a dipole on NOF-H bond
ions pair on NOF atom in one molecule strongly attracts a partially positive hydrogen atom on a different molecule

Question 13

Coordinate bonds

Answer 13

definition: shared e- pair which both comes from the same atom
Properties: act as a covalent bond

Question 14

Valence shell e- par repulsion theory

Answer 14

minimise their repulsion the e- pair repeal each other as far apart as possible
lone pair to lone pair >lone pair to bonding pair> bonding pair to bonding pair

Question 15

electronegativity definition

Answer 15

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

Question 16

Factors which determine how electrongative element is

Answer 16

number of protons
atomic radius
shielding
High electronegativity: high No of protons , low shielding ,low radius

Question 17

model answer for electronegativity

Answer 17

number of protons increases
shielding remains same
therefore ability to attract e- in a covalent bond increases

Question 18

non polar molecules

Answer 18

dipoles act in exactly opposite direction as molecule is symmetrical so dipoles cancel

Question 19

polar molecules

Answer 19

dipoles don’t cancel as molecules is not symmetrical

Question 20

forces between molecule

Answer 20

H-NOF: Hydrogen bonding (strongest)

POLAR: permanent dipole dipole forces

Non-POLAR: induced dipole dipole forces (weakest)

Question 21

Ionic compound formula

Answer 21

+1 charge:
Ammonium (NH4)

-1 Charge:
hydroxide (OH)
nitrate (NO3)
Nitrite (NO2)
hydrocarbonate (HCO3-)
Chlorate(I) (ClO)
Chlorate(V) (ClO3)

-2 charge
carbonate (CO3)
Sulfate (SO4)
Sulphite (SO3)
DIcromate (Cr2O7)

+3 charge
Phospahte (PO4)

Question 22

Covalent bond

Answer 22

Civalent bonds is a shared pair of electrons between 2 atoms