Periodic table

Question 1

What is the atomic radius

Answer 1

The distance between the nucleus and the outermost electron

Question 2

What is the trend with atomic radius in the periodic table

Answer 2

Atomic radius increases down a group and decreases along a period

Question 3

What is electronegativity

Answer 3

The ability of an atom to attract electrons from another compound

Question 4

What is the trend with electronegativity in the periodic table

Answer 4

Increases along a period and decreases down a group

Question 5

Why does electronegativity decrease down a group

Answer 5

Atomic radius increases down a group as there is more electrons, therefore there is a weaker attraction between electrons and the nucleus, so harder to attract electrons

Question 6

What element has the highest electronegativity

Answer 6

Fluorine

Question 7

Is a molecule polar or non-polar when it has a large electronegativity difference

Answer 7

Polar
This is because the atom with the higher electronegativity has a stronger attraction for the bonding pair of electrons.
This means there is an unequal distribution of electrons in the covalent bond, leading to partial charges.

Question 8

Is a molecule with little to no electronegativity difference polar or non-polar?

Answer 8

Non-polar
This is because the electrons are equally shared in the covalent bond.

Question 9

How are ionic bonds formed?

Answer 9

Between a metal and non-metal
The atoms have an even larger electronegativity difference, leading to the metal donating electrons to the non-metal with a larger electronegativity

Question 10

The Pauling scale can be used to determine if a bond is covalent polar, covalent non-polar or ionic, what are the values?

Answer 10

<1.0 - Non-polar covalent
1.0-2.0 - Polar covalent
>2.0 - Ionic

Question 11

What is group 1 and what is their charge?

Answer 11

Alkali metals
+1 charge

Question 12

What is group 2 and what is their charge?

Answer 12

Alkaline metals
+2 charge

Question 13

What are metals in group 3-12 known as and what are their charges?

Answer 13

Transition metals
Charges range from +1-+7
High melting points

Question 14

What is group 13/3 and what are their charges?

Answer 14

Beginning of metalloids
+3 Charge

Question 15

What is group 14/4 and what are their charges?

Answer 15

Metals, one metal and one metalloid
+4/-4 Charge
Likely to form +2 charged ions down the group
E.g. Pb is usually +2 charge
Si and Ge are used as semi-conductors

Question 16

What is group 15/5, 16/6, 17/7 and what are their charges?

Answer 16

Group 5 -3 charge
Group 6 -2 charge
Group 7/Halogens -1 charge

Question 17

What are energy level rules?

Answer 17

1. Electrons fill lowest level orbitals first
   E.g. 1s is filled before 2s
2. There is a maximum of two electrons per orbital
3. Electrons in the same orbital must be opposite spins