2.2.2 Bonding And Structure

Question 1

What is ionic bonding

Answer 1

Electrostatic attraction between positive and negative ions

Question 2

Ionic bonding occurs when?

Answer 2

Metal and non metal
Electrons are transferred from the metal to the non metal

Question 3

Oppositely charged electrons attract through?

Answer 3

Electrostatic forces to become a giant ionic lattice

Question 4

Example of giant ionic lattice

Answer 4

Sodium chloride

Question 5

Ions with a grater charge will have a?

Answer 5

Charge-strength of the ionic bond
It will have a greater attraction and therefore stronger ionic bonding

Question 6

Larger ions with a greater ionic radius will have?

Answer 6

A weaker attraction to the oppositely charged ion because the forces have to act over a greater distace

Question 7

Type of bonding GIL and between what particles
Giant ionic lattice

Answer 7

Ionic and between oppositely charged ions
Positive and negative

Question 8

Solubility
GIL

Answer 8

Soluble to polar substances

Question 9

Conducts when solid? And why?
GIL

Answer 9

No because they are no mobile delocalised electrons
The ions are in fixed structure

Question 10

Conducts when molten/dissolved and why?
GIL

Answer 10

Yes because the ions are now mobile

Question 11

High or low melting/boiling points and why?
GIL

Answer 11

Yes high melting/boiling points because they are strong ionic bods which require energy to break

Question 12

Examples?
GIL

Answer 12

NaCL
MgO

Question 13

Giant covalent lattice
Types of bond and between what particles
GCL

Answer 13

Covalent bonding
Between atoms

Question 14

Solubility?
GCL

Answer 14

Insoluble

Question 15

Conducts when solid? And why? GCL

Answer 15

No because they are no mobile delocalised charged electrons

Question 16

High melting/boiling points? and why? GCL

Answer 16

Yes high because there are strong covalent bonds and requires energy to break

Question 17

Examples? GCL

Answer 17

Diamond and silicon dioxide

Question 18

Giant metallic lattice
Types of bonds? And between what particle?

Answer 18

Metallic bonding and between positive and negative and delocalised electons

Question 19

Solubility? GML

Answer 19

Insoluble

Question 20

Conducts when solid?
And why? GML

Answer 20

Yes because there are mobile delocalised electrons
And it conducts when molten and dissolved

Question 21

High or low melting/boiling points and why?GML

Answer 21

High melting and boiling points because strong metallic bonds so strong attractions so lost of energy is needed to break

Question 22

Examples? GML

Answer 22

Nickel
Magnesium
Copper

Question 23

Simple covalent bonds
Types of bonds and between what particles

Answer 23

Intermolecular forces and between molecules

Question 24

Solubility? SCB

Answer 24

Polar substances dissolve polar substances
Non polar substances dissolve non polar substances

Question 25

Conducts when solid? And why? SCB

Answer 25

No because there are not mobile charged particles

Question 26

Conducts when molten/dissolved SCB

Answer 26

No because there are no mobile charged particles

Question 27

High or low melting/boiling points and why? SCB

Answer 27

Low melting and boiling points because of weak intermolecular forces which require little energy to break

Question 28

Examples? SCB

Answer 28

CO2 Group 7 of the periodic table H20

Question 29

What is a covalent bond

Answer 29

Strong electrostatic attraction between a shared pair of electrons

Question 30

How do they form

Answer 30

Two nonmetals Electrons are shared to gain a full outer shell

Question 31

Enthaply changes?

Answer 31

The heat energy changes stored in a chemical system - H (Triangle h)

Question 32

electonegativity?

Answer 32

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

Question 33

metallic bonding?

Answer 33

electrostatic attraction between a fixed lattice of a positive metal ions and a “sea of declocalised electrons”

Question 34

properties of a metal?

Answer 34

good conductors of heat and electricity high melting and boiling points strong and durable malleable

Question 35

why can a metal conductor electricity?

Answer 35

mobile declosied electrons

Question 36

why do metals have a high melting/boiling points?

Answer 36

they have strong metallic bonds so a strong attraction and require lots of energy to break

Question 37

why are metals malleable

Answer 37

the layers of metal ions can slide over each other

Question 38

general trend across periods for metals

Answer 38

melting points increase more delocalised electrons ions have a greater charge ionic radius decrease so attraction between ions and electrons is stronger

Question 39

polar?

Answer 39

dipoles don’t cancel out non symmetrical

Question 40

non polar?

Answer 40

no dipoles/dipoles cancel out similar electronegativity symmetrical

Question 41

big four with large polarity

Answer 41

fluorine oxygen nitrogen chorine

Question 42

type of bond is permanent dipole dipole

Answer 42

polar bonds

Question 43

explain permanent dipole dipole bonds

Answer 43

when two oppositely charged dipoles attract