Periodic table of elements

Question 1

What are the periods of the periodic table

Answer 1

The rows

Question 2

What are the groups of the periodic table

Answer 2

The columns

Question 3

What is group 1 of the periodic Table known as

Answer 3

Alkali metals

Question 4

What is group 2 of the periodic table known as

Answer 4

Alkaline earth metals

Question 5

What is group 17 of the periodic table known as

Answer 5

Halogens

Question 6

What is group 18 of the periodic table known as

Answer 6

Noble gases

Question 7

What are groups 3 to 12 of the periodic table known as

Answer 7

Transitional metals

Question 8

What are elements 58 to 71 in the periodic table known as

Answer 8

Lanthanoid

Question 9

What are elements 90 to 103 in the periodic table known as

Answer 9

Actinides

Question 10

What are lanthanides

Answer 10

Rare earth metals that are found in small quantities on earth

Question 11

What are actinides

Answer 11

Most wot the known elements used in nuclear reactions and

Question 12

What 4 areas is the periodic table divided into

Answer 12

s,p,d and f block

Question 13

What are the s block elements

Answer 13

Group 1 and 2 elements

Question 14

What are the p block elements

Answer 14

Group 13- group 18

Question 15

What are the d block elements

Answer 15

Group 3- group 12

Question 16

What are the f block elements

Answer 16

Lanthanides and actinides

Question 17

What does the period indicate on the periodic table

Answer 17

The outermost energy level of the elements in that period

Question 18

What happens to the atomic radius from left to right in a given period and why?

Answer 18

It decreases, because there is an increase in protons but the number of energy levels stays the same thus the electrons are drawn more by the nucleus with greater charge so the atom volume shrinks and atomic radii decreases

Question 19

What happens to the atomic radius from top to bottom in a group and why ?

Answer 19

It increases, because as you go down a group the number of energy levels increases thus the number of inner electrons Increases and they shield the outer electrons from the force of attraction of the core thus the atom volume increases so that the atomic radius increases

Question 20

What happens to the melting and boiling point from left to right in a period and why ?

Answer 20

It increases with metals and decreases with nonmetals.

Group 1 metals have one valence electron while group 2 metals have two thus the forces of attraction are stronger in group 2 elements. Group 13 elements have a strong covalent network structure which is stronger than the metal bonding in the group 1 and 2 metals. Group 14 metals have a much stronger covalent structure and bond than group 13 metals. Thus the melting point and boiling point increase for metals across a period from left to right.

Non metals generally exist as simple molecules (diatomic molecules and P4, S8) and mono atomic molecules (Ne and Ar) that are held together by weak intermolecular forces of attraction thus the melting and boiling points are low and they decrease from left to right

Question 21

What happens to the melting and boiling point from top to bottom for a group

Answer 21

It decreases with metals and increases with nonmetals

Because as metal atoms become larger (their atomic radius increases) the forces of attraction between them decrease (the nucleus is further away from the outer electrons and have a weaker force of attraction on them) and thus the melting and boiling points are lower because you need less heat to overcome the forces.

However for non metals it is the opposite because the weak forces of attraction between diatomic molecules increases as the mass of the atom increases

Question 22

What happens to density from left to right across the period

Answer 22

It increases for metals and decreases for non metals

Because metals are tightly packed in a metal crystal and held together by strong forces of attraction between the metal atoms. The more valence electrons the stronger the forces of attraction and the tighter the particles thus the higher the density.

In simple molecules and monatomic molecules there are weak attraction forces between the molecules that causes their density to decrease

Question 23

What are the factors that influence ionisation energy

Answer 23

• The charge of the nucleus
• the distance of the electrons from the nucleus (atomic radius)
• the number of inner level electrons between the outer level electrons and the nucleus (screening effect)
• repulsion forces of electrons in the same orbital

Question 24

What happens to the first ionisation energy from left to right across the period

Answer 24

It increases, because as you move from left to right across a period the number of energy levels stay the same however the charge of the nucleus increases thus the nucleus holds on more tightly to the outer electrons. This means you’ll need more energy to remove the electron thus the ionisation energy increases as you move from left to right across a period

Question 25

What happens to density as you move from top to bottom in a group

Answer 25

The density increases because the atomic mass of the atoms increase

Question 26

What happens to the first ionisation energy as you move from top to bottom in a group

Answer 26

It decreases, this is because as you go down a group a new energy level is added which means there is more inner electrons shielding the outer electrons from the force of attraction of the nucleus and the distance from the nucleus to the outer electrons is larger thus the force of attraction is weaker thus it’s easier to remove an electron.

Question 27

What is the trend between metals and non metals relating to ionisation energies and thus what can we conclude

Answer 27

Metals have low ionisation energies (500-860 kJ.mol-1) whereas nonmetals have high ionisation energies (800-2380 kJ.mol-1). Thus we can conclude that it is expected for metals to form positive ions in chemical reactions

Question 28

Why is the second ionisation energy higher than the first ionisation energy

Answer 28

This is because the positive ion attracts the electrons more strongly

Question 29

What happens to electron affinity as we move from left to right in a period and why?

Answer 29

It becomes more negative, because from left to right nuclear charge increases which would mean that the new added electrons enter the outer Main energy level and they are drawn more strongly by the nucleus.

Question 30

What is trend with metals and non metals relating to electron affinity

Answer 30

Metals have low (low negatives or positive) electron affinities and nonmetals have high (negative) electron affinities, this means that non metals are most likely to for negative ions during a chemical reaction

Question 31

Which group had the highest electron affinity

Answer 31

Halogens because gaining an electron means they reach the octet structure which they are aiming for

Question 32

What happens to electron affinity from top to bottom in a group

Answer 32

It decreases (less negative), because the newly added electrons are further away from the nucleus thus they experience a weaker force of attraction from the nucleus thus the electron affinity decrease

Question 33

What happens to electronegativity for left to right in a period

Answer 33

Increases, because as we move along a period the atoms become smaller and the negative electrons are closer to the nucleus. the positive charge of the nucleus also bigger. This results in valence electrons being held tighter by the nucleus

Question 34

What happens to electro negativity from top to bottom in a group

Answer 34

It decreases, because as more energy levels are added the inner electrons shield the outer electrons from the nucleus positive charge. This means hat the valence electrons are less tightly held and can easily be removed as we go down in a group.

Question 35

In what ratio does oxygen bond with group 1 elements

Answer 35

2:1

Question 36

In what ratio does oxygen bond with group 2 elements

Answer 36

1:1

Question 37

In what ratio does oxygen bond with group 13 elements

Answer 37

2:3

Question 38

In what ratio does oxygen bond with group 14 elements

Answer 38

1:2

Question 39

In what ratio does oxygen bond with group 15 elements

Answer 39

2:5

Question 40

In what ratio does oxygen bond with group 17 elements

Answer 40

2:1

Question 41

What are the characteristics of a metal oxide

Answer 41

They are typical ionic crystalline solids, have high melting and boiling points, and dissolves in water to form bases

Question 42

What are the characteristics of a nonmetal oxide

Answer 42

Simple covalent molecules that dissolve in water to form acids

Question 43

In what ratio does halides bond with group 1 elements

Answer 43

1:1

Question 44

In what ratio does halides bond with group 2 elements

Answer 44

1:2

Question 45

In what ratio does halides bond with group 13 elements

Answer 45

1:3

Question 46

In what ratio does halides bond with group 14 elements

Answer 46

1:4

Question 47

In what ratio does halides bond with group 15 elements

Answer 47

1:3

Question 48

In what ratio does halides bond with group 16 elements

Answer 48

1:2

Question 49

In what ratio do halides bond with halides

Answer 49

1:1

Question 50

What happens when halides form with metals

Answer 50

They form ionic solids

Question 51

What happens when halides bond with non metals

Answer 51

They form simple covalent molecules

Question 52

What do halides end with when bonding

Answer 52

They end with ide