periodicity, Ionisation Energy, And Electronegativity

Question 1

what are the elements in the periodic table ordered by ?

Answer 1

increasing atomic size

Question 2

what happens to the number of shells going down a group ?

Answer 2

increases

Question 3

what happens to the number of shells going along a period ?

Answer 3

stays the same

Question 4

what happens to the number of outer electrons going down a group ?

Answer 4

stays the same

Question 5

what happens to the number of outer electrons going along a period ?

Answer 5

increases

Question 6

what happens to the first ionisation energy going along a period ?

Answer 6

increases

Question 7

what happens to the first ionisation energy down a group ?

Answer 7

decreases

Question 8

what happens to charge going along a period ?

Answer 8

increases

Question 9

what type of bonding is present in H2

Answer 9

covalent molecular

Question 10

what type of bonding is present in Li

Answer 10

metallic lattice

Question 11

what atoms are monatomic

Answer 11

Noble gases (group 0)

Question 12

what type of bonding is present in O2

Answer 12

covalent molecular

Question 13

what type of bonding is present in s8

Answer 13

covalent molecular

Question 14

what type of bonding is present in C60

Answer 14

covalent molecular

Question 15

what elements are covalent networks

Answer 15

B, C (diamonds and graphite), and Si

Question 16

explain metallic bonding

Answer 16

the attraction between a sea of delocalised, negatively charged electrons and positively charged metal ions.
the force of attraction between them causes metallic bonds

Question 17

Explain covalent molecular bonding

Answer 17

The covalent bond is formed by a shared pair of negative electrons electeostatically attracted to the positively charged nucleus between 2 non metal atoms.

Question 18

Explain monatomic bond

Answer 18

Single atoms containing a full outer shell of electrons

Question 19

What is the first ionisation energy ?

Answer 19

The energy required to remove one mole of electrons from a gaseous atom

Question 20

What is the second ionisation energy ?

Answer 20

The energy required to remove a second mole

Question 21

Why does the ionisation energy increase across a period

Answer 21

As the nuclear charge increases the pull of the nucleus on the electrons increases. Meaning the electrons are closer to the nucleus and therefore require more energy to remove

Question 22

Why does the ionisation energy decrease down a group ?

Answer 22

As more shells are added the inner electrons shield the outer electrons from the pull of the nucleus.
Therefore making it easier to remove electrons

Question 23

Why does the electronegativity increase across a period ?

Answer 23

The electronegativity increases because the nuclear charge increases (the higher the positive charge, the stronger the pull for negative electrons)

Question 24

Why does the electronegativity decrease down a group ?

Answer 24

The electronegativity decrease because of inner electrons shielding outer electrons

Question 25

What is electronegativity

Answer 25

The measure of attraction which an atom has for the electrons in the bond