sub shell electron arrangement

Question 1

define orbital

Answer 1

region of space where an electron has a high probability of being formed

Question 2

list the 3 main rules for orbitals

Answer 2

1. orbitals with the lowest energy are filled first
2. fill up s before p
3. fill up unpaired before paired

Question 3

what is the formula for the maximum amount of electrons in a shell

Answer 3

2n^2

Question 4

why do 2 electrons in the same orbital must have opposite spins

Answer 4

electrons repel each other so one must spin up and the other must spin down

(the electrons usually have arrows that point up or down to show the different directions of the spins)

Question 5

name the 4 type of atomic orbitals

Answer 5

s, p, d ,f

Question 6

how many different f orbitals are there and in what shell number are they found in

Answer 6

7 different types of f orbitals and they are found in shells 4 and above

Question 7

how many types of p orbitals are there and what shells contain p orbitals

Answer 7

3 and all shells contain p orbitals except from 1

Question 8

write the orbital arrangement for chromium

Answer 8

1S2 2S2 2P6 3S2 3P6 3D5 4S1

Question 9

why do chromium and copper behave differently in terms of orbital arrangment

Answer 9

the 3d subshell is more stable when half or completely full

Question 10

write the orbital arrangement for copper

Answer 10

1S2 2S2 2P6 3S2 3P6 3D10 4S1

Question 11

describe the development of the understanding of subatomic particles

Answer 11

1913- Bohr put forward that there is a dense positive nucleus that is orbited by negatively charged electrons

1926- Schrodinger used the idea that electrons have similar to properties to waves as well as particles. this lead to quantum mechanics

1932- Chadwick discovered the neutron

Question 12

how many electrons can the first shell hold

Answer 12

2

Question 13

how many electrons can the second shell hold

Answer 13

8

Question 14

how many electron can the third shell hold

Answer 14

18