orbitals

Question 1

total electron capacity in an s orbital

Answer 1

2

Question 2

total electron capacity in a p orbital

Answer 2

6

Question 3

total electron capacity in a d orbital

Answer 3

10

Question 4

isotopes

Answer 4

Atoms of the same element with different numbers of neutrons

Question 5

order that orbitals are filled

Answer 5

s, p, d

Question 6

which elements will have valence electrons ending off in the s orbital?

Answer 6

elements in groups 1 and 2

Question 7

cation

Answer 7

loses an electron to become positively charged

Question 8

anion

Answer 8

gains an electron to become negatively charged

Question 8

reactivity periodic trends

Answer 8

As you go down the periodic table, reactivity increases. As you go left, reactivity increases

Question 8

reactivity

Answer 8

how desperate an electron is to get a full outer shell

Question 8

Atomic radius trends

Answer 8

While elements down each period generally get larger, elements along each period become smaller as more electrons are drawn to the nucleus

Question 8

Ionisation energy

Answer 8

The energy required for an element to lose a valence electron

Question 8

Ionisation energy trends

Answer 8

Ionisation energy incrceases across the period because it becomes harder to lose an electron.

Question 9

electron shielding/clouding effect

Answer 9

the closer the electrons are to the nucleus, the higher the attraction. When sub shells are shielding the force of attraction from the nucleus, the electron has lower ionisation energy.

Question 10

qualities of metals

Answer 10

lustrous, malleanle, ductile, conducts heat and electricity

Question 10

Electronegativity/electroaffinity

Answer 10

the amount of energy required to accept another electron

Question 10

electronegativity trends

Answer 10

the amount of elecctronegativity inrceases across a period as atoms with more valence electrons are more desperate to get electrons into their shell to achieve stability. Electonegativity decreases across a group due to the electron shielding effect (lower elements already have full shells and aren’t as desperate to create another shell).