atomic radius and electronegativity

Question 1

atomic radius

Answer 1

half the distance between two nuclei of a diatomic molecule

Question 2

what is atomic radius influenced by?

Answer 2

• number of occupied energy levels
• core charge

Question 3

core charge

Answer 3

a measure of the net attractive force felt by the valence shell electrons towards the nucleus.

Question 4

how to calculate core charge

Answer 4

the number of protons in the nucleus - the number of electrons in the inner shells

Question 5

trend of core charge

Answer 5

• core charge increases as you move across the period
• core charge stays the same as you move down a group

Question 6

trend of atomic radius

Answer 6

• the atomic radius increases as you move down a group
• atomic radius decreases as you move across a period

Question 7

electronegativity

Answer 7

• the strength with which atoms of an element attract electrons when they are chemically combined with another element.
• a higher electronegativity means that atoms are more able to pull the electrons that are shared in a covalent bond towards their nucleus

Question 8

electronegativity will be high when

Answer 8

• the atomic radius is low
• the core charge on the atoms is high

Question 9

trend of electronegativity

Answer 9

• electronegativity decreases as you move down a group
• electronegativity increases as you move across a period

Question 10

electronegativity explanations structure

Answer 10

1. shells
2. core charge
3. atomic radius
4. conclusion

Question 11

explains why K has a lower electronegativity than Br

Answer 11

1. k = 4 shells, Br = 4 shells
2. k = 1+ Br = 7+
3. atomic radius in K is higher than in Br
4. K has a lower electronegativity because it has the same core change and a higher atomic radius