C2-bonding Mocks

Question 1

Describe the particle arrangement in a solid

Answer 1

Regular pattern, very close vibrates in fixed position

Question 2

Describe the particle arrangement in a liquid

Answer 2

Touching but random close move around each other

Question 3

Describe the particle arrangement in a gas

Answer 3

Completely random, far apart, moves quickly in all directions

Question 4

What are the names of changing from the states of matter

Answer 4

S -> L melting
L -> S freezing
L -> G boiling
G -> L condensing

Question 5

What are the limits of the simple particle model

Answer 5

No forces all represented as spheres all spheres solid

Question 6

What is an ionic bond and give an example

Answer 6

A bond between a metal and non metal-sodium chloride (Nacl)

Question 7

What is a covalent bond and give an example

Answer 7

Open between two or more nonmetals eg diamond

Question 8

What is a metallic bonding give an example

Answer 8

A bond between two or more metals eg- iron (Fe)

Question 9

Describe what happens to form an ionic bond in terms of electrons

Answer 9

Electrons from the outer most shell of metal atom are transferred. Metal atoms lose electrons become positively charged ions. Nonmetals gain electrons and become negatively. Charged ions ions either need an empty or full outer shell to become stable.

Question 10

How would you draw a diagram to show ionic bonding?

Answer 10

Dot and cross diagram, only draw the outer shell. Square brackets. Number eith + - charge outside bracket

Question 11

What is a ionic compound?

Answer 11

A giant lattice structure of ions held together by strong electrostatic forces of attraction between oppositely charged ions

Question 12

What is the empirical formula?

Answer 12

The simplest whole number ratio of atoms or ions in a structure can work out from lattice diagram count each type of ions and simplify

Question 13

What are the advantages and disadvantages of using dot and cross diagram is for ionic bonding

Answer 13

A-shows transfer of electrons
D-doesn’t show ion arrangement in 3D. Space, it doesn’t show relative size of ions

Question 14

What are the advantages and disadvantages of using 3d ball and stick diagram is for ionic bonding

Answer 14

A-shows arrangement of ions in 3D. Space
D-uses sticks instead of forces, which is misleading because forces act in all directions, shows lots of free space which isnt actually there

Question 15

What are the advantages and disadvantages of using 2D ddiagram is for ionic bonding

Answer 15

A-shows the arrangement of Ireland in 1 Layer
D-doesn’t show layers of ions, doesnt show, 3-D arrangement

Question 16

What are the advantages and disadvantages of using 3D diagram is for ionic bonding

Answer 16

A-shows 3-D arrangement in space
D-it’s not to scale, gives no information about the forces of attraction between the ions

Question 17

What are the properties of ionic compounds and what is the reason behind them?

Answer 17

High, melting and boiling points-strong electrostatic force of attraction between oppositely charged ions which need lots of energy to overcome

Can conduct electricity when melted or dissolved in water, but not when solid -the ions are f free to move charge can flow freely

Question 18

What is a covalent bond?

Answer 18

When electrons are shared between nonmetal atoms

Question 19

Go to the examples of small molecules

Answer 19

Water, oxygen and carbon dioxide

Question 20

Give some examples of giant covalent structures

Answer 20

Diamond and silicone dioxide

Question 21

Describe the properties of substances with giant covalent, structures and why

Answer 21

Solids with very high melting points-many strong covalent bonds between atoms must be broken, which requires lots of energy

All atoms in the giant covalent structure are bonded to each other by strong covalent bonds -don’t conduct, naughty little close electrons or ions that are free to move to carry charge (except graphite)

Question 22

Give some properties of small molecules, and why

Answer 22

Gases or liquids with low melting and boiling points-the weak intermolecular forces between molecules are overcome, know the strong covalent bonds between atoms (intra) -does not require much energy

Don’t conduct electricity-have no charge

Question 23

What is a polymer?

Answer 23

Very large molecule is made up of many repeating units joined by covalent bonds-polly machines held together by intermolecular forces (used to make ip plastic)

Question 24

Give some properties of polymers, and why

Answer 24

Strong-long molecules
Higher melting and boiling points in small molecules solid at room temperature

Question 25

How would you draw a polymer?

Answer 25

Eg polyethene Square, brackets show bonding between carbon and hydrogen n represents large number of how many times repeated

Question 26

Describe the structure and properties of diamond

Answer 26

Strong, covalent structure-every carbon atom, forms for strong covalent bond with other carbon atoms Strong-requires lots of energy to break No delocalised, electrons or Ions to carry charge TETRAHEDRAL

Question 27

What are the advantages and disadvantages of using dot and cross diagram is for covalent bonding

Answer 27

A-show the transfer of electrons, shows which atom bonding electrons came from D-doesn’t show how atoms are arranged in 3-D. Space, doesn’t show relative size or atom

Question 28

What are the advantages and disadvantages of using 3D ball and stick diagram is for covalent bonding

Answer 28

A-shows shape of molecule, shows arrangement of atoms in 3D. Space D-uses sticks for bonds not forces, atoms of placed far apart but in reality the gaps arer smaller

Question 29

What are the advantages and disadvantages of using 3D diagram is for covalent bonding

Answer 29

A-shows the 3-D arrangement in space D- not to scale, give no information about the forces of attraction between atoms

Question 30

What are the advantages and disadvantages of using 2D diagram is for covalent bonding

Answer 30

A-shows what atoms are in a molecule and how they are connected D-Doesn’t show the relative size of the atoms and bonds, doesn’t show the 3-D arrangement in space.

Question 31

Describe the bonding and structure in graphite

Answer 31

Made up of only carbon atoms Forms hexagonal rings, arranged in layers Forms strong, covalent bonds with three other carbon atoms Left with one spare electron, which is delocalised and free to move through the layers

Question 32

Why can graphite conduct electricity?

Answer 32

Each carbon atom has one delocalised electron which is delocalised and free to move and carry electrical charge through the layers

Question 33

Why is graphite slippery?

Answer 33

It has layers with weak intermolecular forces between them, which don’t require much energy to overcome

Question 34

What is graphene and what is it used for

Answer 34

It is a single layer of graphite. It’s properties make it useful in electronics and composites

Question 35

What are the properties of graphene

Answer 35

Strong covalent bonds between carbon atoms-very strong with high melting and boiling points-take a lot of energy to break the strong covalent bonds Only bonded with 3 other carbons. -conductor of electricity

Question 36

What is fullerene?

Answer 36

Molecules of carbon atoms with hollow shapes. Based on hexagonal rings (can sometimes have rings with 5 or 7 carbon atoms) can be arranged as a tube (nanotube) or ball ( buckminster fullerene c60)

Question 37

What is the properties of carbon nano tube?

Answer 37

Cylindrical fullerene with very high length to diameter ratio. They have high tensile strength so difficult to break. Used in nanotechnology electronics and materials.

Question 38

What are the properties of Buckminister fullerene?

Answer 38

Molecule made of 60 carbon atoms covalently bonded into a spherical shape. Weak intermolecular forces between molecules. Low melting point, and slippery lubricant and for drug delivery.

Question 39

Describe the structure of metals

Answer 39

Giant structures of atoms with strong metallic bonds. Most metals have high, melting and boiling points. Requires a lot of energy to overcome.

Question 40

What are the structure of pure metals?

Answer 40

Atoms arranged in layers Layers can slide over each other Pure metals can be bent and shaped (malleable) Pure metals can be too soft

Question 41

Describe the structure of alloys

Answer 41

If we mix pure metals with other elements, we can make an alloy Atoms of different elements are different sizes Distort, layers Can’t slide over one another easily More force is required, makes alloys harder and stronger than pure metals

Question 42

What happens to metas that causes metalic bonding

Answer 42

Metal is made up of giant structure of atom is arranging a regular pattern electrons in outer shell of metal atoms delocalised electrons

Question 43

Why can metals conduct electricity?

Answer 43

Sea of delocalised electrons, free to move through the layers

Question 44

Why are metals good conductors of thermal energy

Answer 44

Delocalised electrons transfer energy?

Question 45

What causes metallic bonding?

Answer 45

The sharing of delocalised electrons

Question 46

What is a nano particle

Answer 46

Particles between 1-100 nm inside, made up of a few hundred atoms

Question 47

What is the size of an atom

Answer 47

1 x 10 to the -10 m

Question 48

What is the size of a nanoparticle

Answer 48

1x 10 to the -9 m - 1x 10 to the -7 m

Question 49

What is the size of a fine particles (pm2.5)

Answer 49

1 x 10 to the -7 - 2.5 x 10 to the -6 m

Question 50

What is the size of coarse particles? (Pm10)

Answer 50

2.5 x 10 to the -6m - 1 x 10 to the -5 m

Question 51

What are the uses of nano particles?

Answer 51

Medicine Electronics Cosmetic Suncream Deodorant Catalysts

Question 52

What are the risks of nano particles?

Answer 52

. Can we breathe in . Can enter cells . Can catalyse harmful reactions . Toxic substances can bind to them due to the large surface area to volume ratio.

Question 53

How would you workout the surface area to volume ratio of 1 cm cube

Answer 53

Sa- 6 x 1 x 1 = 6cm Vol- 1x 1 x 1 =1cm Sa:vol- 6/1=6cm

Question 54

How would you workout the surface area to volume ratio of 10 cm cube?

Answer 54

Sa-6x10x10=600cm Vol=10x10x10=1000cm Sa:vol= 600/1000=0.6cm