Bonding: Ionic/Covalent/Metallic

Question 1

What is ionic bonding?

Answer 1

bonding resulting from electrostatic attraction between oppositely charged ions

Question 2

where is the electron transferred from and to in an ionic bond?

Answer 2

metal to non-metal

Question 3

what is the name for positively charged ion?

Answer 3

cation

Question 4

what is the name for negatively charged ion?

Answer 4

anion

Question 5

explain the ionic bonding in NaCl

Answer 5

• sodium has 11 electrons and arrangement of 1s2, 2s2, 2p6, 3s1
• chlorine has 17 electrons and arrangement of 1s2, 2s2, 2p6, 3s2, 3p5
• the 3s1 electron from sodium is transferred to the outer main level of chlorine
• sodium becomes positively charged since it has lost an electron
• chlorine becomes negatively charged since it has gained an electron
• these ions are attracted to each other and to the other oppositely charged ions by electrostatic attraction

Question 6

what type of structure do ionic compounds have?

Answer 6

lattic structure

Question 7

what state are ionic compounds at rtp?

Answer 7

solid

Question 8

do ionic compounds have high or low mp? and why?

Answer 8

high mp - high amount of energy is required to break bonds in lattice

Question 9

in what state do ionic compounds conduct electricity? and why?

Answer 9

molten - ions are free to move

Question 10

why are ionic compounds brittle?

Answer 10

when lattice of alternating ions is displaced, the ions repel each other so break apart

Question 11

what is metallic bonding?

Answer 11

a lattice of positively charged ions in a sea of ‘delocalised electrons’

Question 12

why are metals good conductors of electricity?

Answer 12

delocalised electrons are free to move through structure

Question 13

are metals good or bad conductors of heat?

Answer 13

good - high thermal conductivity (energy spread by vibration of closely packed ions and electrons moving through structure)

Question 14

why do metals tend to be strong?

Answer 14

no individual bonds to break because of the electrons throughout the solid

Question 15

how does charge affect the strength of the metal?

Answer 15

the greater the charge, the stronger attraction because there are more delocalised electrons so more electrostatic attraction

Question 16

how does the size of a metal affect its strength?

Answer 16

the smaller the ion, the stronger the nuclear charge because electrons closer to nucleus

Question 17

why are metals malleable and ductile?

Answer 17

layers of ions can easily slide over each other

Question 18

why do metals have high bp and mp?

Answer 18

giant structure - so strong attraction between ions and electrons - therefore high amount of energy to overcome attraction

Question 19

what is a covalent bond?

Answer 19

a shared pair of electrons

Question 20

explain the covalent bonding in methane

Answer 20

• methane is a compound of hydrogen and carbon
• carbon has 6 electrons and an electron arrangement of 1s2 2s2 2p2
• hydrogen only has one electron - 1s1
• therefore four atoms of hydrogen are required to fill the outer main level of carbon
• four electrons from carbon and 1s1 electron from four hydrogen atoms are shared
• formula: CH4

Question 21

what is another term for co-ordinate bonding ?

Answer 21

dative covalent bonding

Question 22

what is co-ordinate bonding?

Answer 22

when both electrons is donated by an atom in a covalent bond

Question 23

what is the term to describe the atom which accepts the electron pair?

Answer 23

electron-deficient

Question 24

what type of electron pair is donated?

Answer 24

lone pair