1.2 atomic orbitals, electronic configurations & the periodic table

Question 1

orbitals

Answer 1

stationary waves in an atom, vibrate in time
can hold a maximum of 2 electrons
spdf

Question 2

principle quantum number

Answer 2

n
indicates an electron’s energy level

Question 3

angular momentum quantum number

Answer 3

l
indicates the shape of the subshell
values from 0 to n-1

Question 4

magnetic quantum number

Answer 4

Ml
indicates the orientation of the orbital
values between -l and +l

Question 5

magnetic spin quantum number

Answer 5

Ms
indicates the direction of spin
values of either -1/2 or +1/2

Question 6

s subshell

Answer 6

l = 0
holds 2 electrons maximum
1 value of Ml
spherical

Question 7

p subshell

Answer 7

l = 1
holds 6 electrons maximum
3 values for Ml
dumbbell shaped

Question 8

d subshell

Answer 8

l = 2
holds 10 electrons maximum
5 values for Ml

Question 9

f subshell

Answer 9

l = 3
holds 14 electrons maximum
7 values for Ml

Question 10

degenerate

Answer 10

orbitals of the same subshell have equal energy

Question 11

pauli exclusion principle

Answer 11

no 2 electrons of the same atom can have the same set of 4 quantum numbers

Question 12

what does the pauli exclusion principle mean?

Answer 12

orbitals hold a maximum of 2 electrons
each electron within an orbital must have opposite spins

Question 13

aufbau principle

Answer 13

electrons fill orbitals in order of increasing energy

Question 14

hund’s rule

Answer 14

when degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts

Question 15

subshell stability

Answer 15

half-filled and fully-filled subshells are more stable than other incomplete subshells

Question 16

vsepr theory step 1

Answer 16

take the number of valence electrons on the central atom

Question 17

vsepr theory 2

Answer 17

add an electron for each attached atom

Question 18

vsepr theory 3

Answer 18

add electrons for negative charges
subtract electrons for positive charges

Question 19

vsepr theory 4

Answer 19

divide by 2 for the number of electron pairs

Question 20

electron pair repulsion

Answer 20

negatively charged pairs repel each other so arrange to minimise repulsion and maximise separation

Question 21

highest electron pair repulsion

Answer 21

lone pair-lone pair

Question 22

lowest electron pair repulsion

Answer 22

bonding pair-bonding pair

Question 23

dative covalent bonds

Answer 23

form when both electrons in a covalent bond are from the same atom

Question 24

linear shaped molecules

Answer 24

2 bonding electron pairs
180° bond angle

Question 25

trigonal planar shaped molecules

Answer 25

3 bonding electron pairs 120° bond angle

Question 26

tetrahedral shaped molecules

Answer 26

4 bonding electron pairs 109.5° bond angle

Question 27

angular shaped molecules

Answer 27

2 bonding electron pairs 2 lone electron pairs 104.5° bond angle

Question 28

trigonal pyramidal shaped molecules

Answer 28

3 bonding electron pairs 1 lone electron pair 107° bond angle

Question 29

trigonal bipyramidal shaped molecules

Answer 29

5 bonding electron pairs · 120° equatorial bond angle · 90° eq/ax bond angle · 180° axial bond angle

Question 30

octahedral shaped molecules

Answer 30

6 bonding electron pairs 90° bond angle

Question 31

square pyramidal shaped molecules

Answer 31

5 bonding electron pairs 1 lone electron pair 82° bond angle

Question 32

square planar shaped molecules

Answer 32

4 bonding electron pairs 2 lone electron pairs 90° bond angle