The Periodic Table And Bonding

Question 1

Loss of electrons

Answer 1

Oxidation

Question 2

Gain of electrons

Answer 2

Reduction

Question 3

Ions

Answer 3

Charged particles, formed when atoms lose or gain electrons.

Ions always have the same number of protons and neutrons.

Question 4

Electronic transfer

Answer 4

The relocation of electrons from one atom to another.

Question 5

Ionic bonding

Answer 5

Oppositely charged ions that are strongly attracted to each other (strong electrostatic attraction between ions with positive and negative charges).
Electrostatic - charge unchanging

Question 6

Physical properties of ionic substances - electrical conductivity (solid)

Answer 6

Solid ionic substances do not conduct electricity.
Particles in a solid are tightly packed.
In an ionic solid, the positive and negative ions alternate in a tightly packed structure.
Electricity = moving charged particles
In an ionic solid, the ions cannot move freely (although they do vibrate)

Question 7

Physical properties of ionic substances - electrical conductivity (liquid)

Answer 7

Ionic substances dissolved in water do conduct electricity. Dissolved ionic substance (state of matter = liquid/soluting)
When dissolved in water, the ions are able to move freely, swapping places with the water and each other.
The solution conducts electricity.
Ionic substances in liquid from (melted/molten) also conduct electricity. This is possible because ions are free to move with each other.

Question 8

Physical properties of ionic substances - melting point

Answer 8

Mp = temperature at which a substance changes from a solid to a liquid.
Ionic solids did not melt when using a Bunsen flame.
An ionic solid has a strong attraction between positive and negative ions. Lots of heat energy is required to overcome the attraction and separate the ion into liquid state.

Question 9

Simple ions

Answer 9

Hydrogen         H+
Silver                Ag+
Zinc                  Zn^2+
Copper(||)       Cu^2+
Iron(||)              Fe^2+
Iron(|||)             Fe^3+
Lead(|||)           Pb^3+

Question 10

Complex ion

Answer 10

Ammonia NH4+

Hydroxide OH-

Nitrate NO3-

Carbonate CO3^2-

Sulphate SO4^2-

Question 11

Covalent bond

Answer 11

The sharing of a pair of electrons between two atoms

Question 12

Covalent bonding

Answer 12

A strong attraction between the bonding pair of electrons and the nuclei of the atoms involved in the bond.

Question 13

Simple covalent structure

Answer 13

Simple covalent structures apply to molecules that can be drawn in a dot cross diagram.
Simple covalent = simple molecular structure

Question 14

Electrical conductivity of simple covalent

Answer 14

Substances with simple molecular structures do not conduct electricity when solid.
No free electrons and no ions are able to move.

Substances with simple molecular structures do not conduct electricity when liquid.
No electrons are present.

Question 15

Boiling point of simple covalent

Answer 15

Low - little heat energy was required to change state from liquid to gas therefore intermolecular forces of attraction are weak.
! Covalent bonds do not break during a change of state.

Question 16

Boiling points of simple covalents

Answer 16

Low - substances with simple molecular structures have low melting points.
Little heat energy is needed to change the arrangement of particles from solid to liquid because the intermolecular forces are weak.
The larger the covalent molecule, the stronger the intermolecular forces of attraction.

Question 17

Mono

Answer 17

1

Question 18

Di

Answer 18

2

Question 19

Tri

Answer 19

3

Question 20

Tetra

Answer 20

4

Question 21

Penta

Answer 21

5

Question 22

Hexa

Answer 22

6

Question 23

Giant covalent structures

Answer 23

Made of many atoms held together by covalent bonds.

Question 24

Giant covalent structure example 1

Answer 24

Carbon, graphite
Graphite is made entirely of carbon atoms.
Within a layer, carbon atoms are held together by strong covalent bonds.
The layers are held together by weak forces of attraction.
Each carbon atom is bonded to 3 other carbon atoms (each layer is flat).

Question 25

Physical property no. 1 of example 1 of giant covalent structures (carbon, graphite)

Answer 25

Does conduct electricity when solid.
There are delocalized electrons which are able to move. E.g. carbon has 1 delocalized electron because there are only 3 atoms at the end of a bond - there needs to be 4.

Question 26

Physical property no. 2 of example 1 of giant covalent structures (carbon, graphite)

Answer 26

Soft
By applying a force, layers of carbon atoms slide over one another.
Forces of attraction between layers are weak.

Question 27

Physical property no. 3 of example 1 of giant covalent structures (carbon, graphite)

Answer 27

Melting/boiling point - high
To change state, covalent bonds must be broken.
Lots of heat energy is required. Therefore high melting/boiling point.

Question 28

Giant Covalent Structure example 2

Answer 28

Carbon, diamond

Each carbon atom is bonded to 4 other carbon atoms in a tetrahedral shape.

Question 29

Physical property no. 1 of example 2 of giant covalent structures (carbon, diamond)

Answer 29

No electrical conductivity

Every electron for the carbon atoms is involved in bonding therefore no delocalized electrons.

Question 30

Physical property no. 2 of example 2 of giant covalent structures (carbon, diamond)

Answer 30

Hard

The tetrahedral structure of covalent bonds is very strong. Therefore not affected by applying a force.

Question 31

Physical property no. 3 of example 2 of giant covalent structures (carbon, diamond)

Answer 31

Melting/boiling point is high.

Strong covalent bonds must be broken in order to change state. Therefore lots of heat energy is needed.

Question 32

Allotrope

Answer 32

An element that has different structures (the atoms of the element can be bonded in different arrangement).

Question 33

Buckminsterfullerene

Answer 33

Made entirely of carbon atoms, with chemical formula C60 - macromolecule.
A solid at room temperature.
Carbon atoms in the structure of C60 are held together by strong covalent bonds.
The giant structures are held together by weak forces of attraction.

Question 34

Physical property no. 1 of the buckminsterfullerene

Answer 34

No electrical conductivity for multiple C60.

Each C60 can conduct within the molecule but delocalized electrons cannot travel to a different C60.