The periodic table

Question 1

What are some properties of group 1 Alkali metals

Answer 1

Soft
Highly reactive
Low melting points
Form soluble salts

Question 2

Where are the d - block elements

Answer 2

3-12

Question 3

What are non - metal properties

Answer 3

poor conductors
not hard
solid , liquid or gas at room temperature

Question 4

At room temperature what are florine and chlorine

Answer 4

Gasses

Question 5

At room temperature what is Br

Answer 5

liquid

Question 6

At room temperature what is I

Answer 6

solid

Question 7

What are the properties of the Noble gasses

Answer 7

Highly reactive
Gases

Question 8

What is the first row of the f-block called

Answer 8

Lanthanides

Question 9

What is the second row of the f-block called

Answer 9

Actinides

Question 10

What are the properties of f-block

Answer 10

Complex and heavy metals
Highly reactive
High melting and boiling points

Question 11

Elements in the same period have the same number of

Answer 11

shells

Question 12

Across a period
Charge of nucleus …
Atomic Radius …

Answer 12

Increases
Decreases

Question 13

Where are the metals and non-metals located

Answer 13

metals - left
non metals - right

Question 14

Definition of Ionisation Energy

Answer 14

The energy needed to remove one mol of an electron from a mole of gaseous atoms of ions

Question 15

Atomic radius and Ionisation Energy are

Answer 15

Inversely Proportional

Question 16

What happens down a group between
Atomic radius :
Ionisation Energy :

Answer 16

Increases
Decrease

Question 17

What happens across a period between
Atomic Radius
Ionisation Energy

Answer 17

Decrease
Increase

Question 18

Define electron affinity

Answer 18

The energy released when one mole of an atom gains an electron to form a negatively charged ion

Question 19

Explain the trend between electron affinity down the group

Answer 19

decreases

Question 20

Explain the trend between electron affinity across a period

Answer 20

increases

Question 21

Define Electronegativity

Answer 21

The ability of an atom to attract a pair of bonded electrons

Question 22

Electronegativity decreases down a group because

Answer 22

nuclear charge increases
increased shielding
large atomic radius due to increase in electron shell

Question 23

Electronegativity increased across a period because

Answer 23

Effective nuclear charge increases
Stronger attraction between the nucleus and the shared pair of electrons

Question 24

What decreases as you go down group 1

Answer 24

ionisation energy

Question 25

What increases as you go down group 1

Answer 25

reactivity number of occupied energy levels

Question 26

What increases down group 17

Answer 26

number of occupied energy levels

Question 27

What decreases down group 17

Answer 27

electron affinity reactivity

Question 28

Define first ionisation energy

Answer 28

minimum energy required to lose one mole of electrons from one mole of gaseous atoms to produce one mole of gaseous ions

Question 29

Explain why the first ionisation energy decreases down a group (3)

Answer 29

• Going down a group atomic radii increases and electrons occupy higher energy levels • Electrons in higher energy levels have a weaker attraction to the nucleus. • Less energy is required in order to remove an electron

Question 30

Explain why first ionisation energy increases across a period

Answer 30

Going across there are more protons in the nucleus and more electrons occupying the outermost energy level (effective nuclear charge) • A greater number of electrons in the outermost energy level results in a stronger attraction to the nucleus • More energy is required in order to remove an electron

Question 31

Atomic radius

Answer 31

Increases down a group decreases across a period

Question 32

Define First Electron affinity

Answer 32

the amount of energy released when a neutral atom gains an electron to form a negatively charged ion

Question 33

Why does First electron affinity decrease down a group

Answer 33

The atomic radius becomes larger , the attraction for an additional electron is less , since the effective nuclear charge is reduce due to increased shielding

Question 34

Why does electron affinity increase across a period

Answer 34

Elements across a period have a higher effective nuclear charge. Stronger attraction between the added electron and the nucleus

Question 35

What are the 6 characteristic properties of transition elements

Answer 35

• Variable oxidation states • High melting points • Magnetic properties • Catalytic properties • Formation of coloured compounds • Formation of complex ions

Question 36

if the ionisation number is 2+ what its oxidation number

Answer 36

+2

Question 37

What is a transition element

Answer 37

element with a partially filled d-subshell

Question 38

what is effective nuclear charge

Answer 38

more electrons in shells

Question 39

What type of metals have low EA

Answer 39

metals

Question 40

What type of metals have a high EA

Answer 40

non-metals

Question 41

Why do metals have low electronegativities

Answer 41

because they lose electrons easily

Question 42

why do non-metals have high electronegativities

Answer 42

as they gain electrons to fill their outer shell

Question 43

What is the trend in melting points ?

Answer 43

Increase across a period until group 14 then decrease

Question 44

What is the trend in metallic character

Answer 44

Increases down a group Decreases across a period

Question 45

What is the acidic state of sodium oxide Na2O

Answer 45

Basic

Question 46

What is the acidic state of magnesium oxide Mgo

Answer 46

Basic

Question 47

What is the acidic state of Aluminium Oxide Al2O3

Answer 47

Amphoteric

Question 48

What is the acidic state of Silicon Oxide SiO2

Answer 48

acidic

Question 49

What is the acidic state of Phosphorus

Answer 49

Acidic

Question 50

What is the acidic state of sulfur oxide SO2

Answer 50

acidic

Question 51

What is the acidic state of chlorine oxide

Answer 51

Acidic