Trends Periodic Table

Question 1

Most Reactive Chemical Groups

Answer 1

1 and 7

Question 2

Period

Answer 2

Horizontal across periodic table. Elements similar chemical properties

Question 3

Group Def.

Answer 3

Verticle periodic table

Question 4

Metal Def.

Answer 4

Good conductor of heat/electricity

Question 5

Non-metal def.

Answer 5

Poor conductor of heat/electricity

Question 6

Metalloid Def.

Answer 6

Part metal, part non. Conductor of heat of standard between metal and non-metal

Question 7

Effective Nuclear Force Depends On

Answer 7

No. of protons in nucleus, shielding effects of orbits closer to nucleus and distance from nucleus

Question 8

Effective Nuclear Charge (Zeff)

Answer 8

Nuclear charge felt by an electron when both the effective nuclear charge and shielding effect into account

Question 9

Zeff across period

Answer 9

Increases (as atomic number does and screening remains the same)

Question 10

Zeff down group

Answer 10

Decreases (as screening increases)

Question 11

Atomic Radius Def.

Answer 11

Half the distance between 2 nuclei if 2 adjacent atoms

Question 12

Atomic Radius across period

Answer 12

Decreases

Question 13

Atomic Radius down group

Answer 13

decreases

Question 14

Ionic Radius Change during anion Formation

Answer 14

Increases. Additional electron causes others to be pushed outwards by repulsive force (nuclear charge in same)

Question 15

Ionic Radius change during cation formation

Answer 15

Decreases. Electron removed causes force repelling electrons outwards to diminish

Question 16

Ionic Radius of dipositive ions are smaller then Ionic radius of unipositive ions that are isoelectronic because…

Answer 16

Dipositive ion has bigger nuclear charge

Question 17

Ionic radii of dinegative ions are bigger the isoelectronic uninegative ions because….

Answer 17

Uninegative has less screening = bigger nuclear charge

Question 18

1st Ionisation Energy (kJ/mol)

Answer 18

Min. energy required to remove the outermost electron from a ground atom in gaseous state

Question 19

Ionisation energy across period

Answer 19

Increases

Question 20

Ionisation Energy down group

Answer 20

decreases

Question 21

Electronegativity Def.

Answer 21

Ability of an atom to attract electrons towards itself in a chemical bond

Question 22

Electron Affinity Def.

Answer 22

The negative energy change that occurs when an electron is accepted by a neutral gaseous atom

Question 23

Relationship between electron affinity and atoms accepting electrons

Answer 23

Greater positive electron affinity, greater chance of accepting electron

Question 24

Relationship between heat change and electron affinity

Answer 24

• x kJ/mol = + x kJ/mol

Question 25

Why is F the most electronegative element

Answer 25

High nuclear charge, little shielding. High electron affinity and high ionization energy

Question 26

Most electronegative elements

Answer 26

F > O > N > C