Structure And Bonding

Question 1

What’s ionic bonding

Answer 1

Metal and non metal

Question 2

What’s room temp

Answer 2

25 C

Question 3

What’s covalent bonding

Answer 3

Non metal and non metal
Pair of electrons shared
Strong bonds

Question 4

What’s metal made of

Answer 4

Positive atoms or ions around sea of delocalised electrons

Question 5

Why can metal conduct electricity

Answer 5

Electrons are free to move

giant structure close packed
made up of atoms
with delocalized and free electrons
so electrons can move / flow through the metal

Question 6

Difference of alloy and pure metal

Answer 6

Alloy- has electrons and ions but has another metal or non metal

Question 7

Describe a pure metal

Answer 7

Has layers
= can slide across each other
= soft

Question 8

Describe an alloy

Answer 8

Has distorted layers
= can’t slide
= hard

Question 9

Describe ionic compounds structure

Answer 9

Giant ionic lattice
high melting point
= high boiling point
= only conduct when molten or dissolved
( ions need to be free to move )

Question 10

Describe simple covalent compounds structure eg water, oxygen

Answer 10

Covalent bonding
= low melting points
= low boiling points
= don’t conduct electricity

Question 11

Describe giant covalent compounds structure eg graphite, diamond

Answer 11

Giant covalent structure
= high melting points
= high boiling points
= don’t conduct electricity
= don’t dissolve

Question 12

Describe diamond structure

Answer 12

Made of carbon
= create giant covalent lattice
Each carbon makes 4 bonds
- hard

Question 13

Describe graphite structure

Answer 13

Made of carbon
= giant covalent
Each carbon bonds 3 times
- soft
- conducts electricity

Question 14

Compare graphite and diamond

Answer 14

• both made of pure carbon
• graphite is made of 3 bonds
• diamond is made of 4 bonds
• graphite is soft
• diamond is hard

Question 15

Compare carbon nanotubes and buckminster fullerene

Answer 15

• Both made of pure carbon
• Both hard
• Both have 3 carbon bonds
• buck used for lubricant
• both used for drug delivery

Question 16

Describe nanotechnology

Answer 16

Very small
= increasing surface area
= different properties
= used for medicine drug delivery

Question 17

Why can metals bend

Answer 17

Made of layers
= atoms can slide over each other

Question 18

Why is graphite soft

Answer 18

Contains layers that’s slide over each other
= between layers there are only weak forces

Question 19

Why is diamond hard

Answer 19

Each atoms forms 4 covalent bonds
= covalent bonds are very strong

Question 20

Why does graphite conduct electricity

Answer 20

Has delocalised electrons which move through whole structure and carry the charge

Question 21

Why can sodium chloride solution conduct electricity

Answer 21

there are ions in sodium chloride
which can move or carry the current / charge

Question 22

Disadvantage of copper

Answer 22

copper metal is in demand
copper is expensive

Question 23

Why is an alloy harder than pure metal

Answer 23

Atoms have different sizes
Have distorted layers
= harder for layers to slide
= elements can’t move through structure

Question 24

Copper can be extracted from solutions of copper salts by adding iron

Answer 24

Iron more reactive
= copper is displaced

Question 25

How can you tell that copper is a transition metal and aluminium is not a transition metal from the position of each metal in the periodic table?

Answer 25

copper is in the central block of the periodic table
whereas aluminium is in Group 3 of the periodic table

Question 26

Describe the structure and bonding in metals

Answer 26

Giant structure of atoms/ ions with selects listed electrons

Question 27

Reasons for low boiling point

Answer 27

• made of small molecules
  = weak intermolecular forces
  = little energy required to overcome intermolecular bonds

Question 28

Describe alpha particle scattering experiment

Answer 28

• hammered gold into foil and fired tiny alpha particles at foil
• particles either went through atom or bounced off
• particles that went through proved atom mainly made of empty space not electrons
• some deflected meant centre must be positive

Question 29

Why does boiling point increase

Answer 29

Relative mass increases
Molecules become larger
= stronger intermolecular forces
= more energy required to overcome intermolecular forces

Question 30

Describe reactivity of halogens

Answer 30

As you go down become further from nucleus
= nucleus has less attraction to outer shells
= electron gained less easily

Question 31

Adv of using burette

Answer 31

Can measure variable volumes
Can add solution drop by drop

Question 32

Adv of using a burette

Answer 32

Can add solution drop by drop
Can measure variable volumes

Question 33

Reason for high boiling point

Answer 33

giant structure
(with) strong (electrostatic) forces of attraction between (oppositely charged) ions
(so) large amounts of energy are needed to break the bonds / forces

Question 34

Describe a fullerene

Answer 34

Tubular or hollow spherical molecules held together by covalent bonds
3 covalent bonds per atom
= 1 spare electron per carbon atom
= electrons can flow through structure
= can conduct electricity