Atomic Orbitals & The Periodic Table

Question 1

How do electrons behave within the atom?

Answer 1

as standing waves

Question 2

What are standing waves?

Answer 2

waves that vibrate in time but do not move in space

Question 3

What is the max no of electrons in orbitals?

Answer 3

2

Question 4

How many quantum numbers are there?

Answer 4

4

Question 5

What are the four quantum numbers?

Answer 5

• principle quantum number
• angular momentum quantum number
• magnetic quantum number
• spin magnetic quantum number

Question 6

How is the principle quantum number defined?

Answer 6

n

Question 7

What does n=1 represent?

Answer 7

the shell closest to the nucleus

Question 8

What can be said about the greater the value of n?

Answer 8

the greater the value of n, the higher the energy level and further from the nucleus the electron must be

Question 9

What is the second quantum number defined by?

Answer 9

l

Question 10

What does the second quantum number determine?

Answer 10

the shape of the subshell

Question 11

What are the range of values for l?

Answer 11

l has values ranging from 0 to n-1

Question 12

How is the magnetic quantum number defined?

Answer 12

ml

Question 13

What does the magnetic quantum number define?

Answer 13

the number of orbitals

Question 14

What are the range of values for ml?

Answer 14

-l to l

Question 15

What can be said about the shape of s orbitals?

Answer 15

they are spherical in shape

Question 16

What happens to the size and energy of an s orbital as the value of n increases?

Answer 16

size and energy increase

Question 17

How many possible orientations of p orbitals are there?

Answer 17

3

Question 18

How many d orbitals are there?

Answer 18

5

Question 19

How many orientations do f orbitals have?

Answer 19

7

Question 20

What does the magnetic spin number do?

Answer 20

determines the direction of electron spin

Question 21

What ways can electronic configuration be expressed?

Answer 21

• using quantum numbers
• orbital box notation
• spectroscopic notation

Question 22

What is the Aufbau principle?

Answer 22

electrons fill orbitals in order of increasing energy

Question 23

What is Hund’s rule?

Answer 23

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

Question 24

What shell has more energy the 4s or 3d orbital?

Answer 24

3d has more energy than the 4s

Question 25

What block are groups 1&2 in?

Answer 25

the s block

Question 26

What block are groups 3& 8 in?

Answer 26

p block

Question 27

What block are transition metals in?

Answer 27

d block

Question 28

What is ionisation energy?

Answer 28

the energy required to remove 1 mole of electrons from 1 mol of atoms in the gaseous state

Question 29

What happens to ionisation energy across a row?

Answer 29

it increases due to an increase in nuclear charge

Question 30

What happens to ionisation energy down a period?

Answer 30

decreases down a period due to an increased shielding effect

Question 31

What does VSEPR stand for?

Answer 31

valence shell electron pair repulsion theory

Question 32

How is the number of electron pairs calculated?

Answer 32

e pairs=no. of outer e pairs+no. of bonded atoms/2

Question 33

What is the shape of molecules due to?

Answer 33

the number of electron pairs or group of electron pairs

Question 34

What is the relationship between lone pairs and bonded pairs?

Answer 34

the pairs are more repulsive than bonded pairs

Question 35

What is the trend in repulsivity?

Answer 35

bonded to bonded< bonded to lone

Question 36

Linear

Answer 36

2 electron pairs

180 degrees

Question 37

Trigonal planar

Answer 37

3 electron pairs

120 degrees

Question 38

Tetrahedral

Answer 38

4 electron pairs

109.5 degrees

Question 39

Trigonal bipyramidal

Answer 39

5 electron pairs

90, 120, 180 degrees

Question 40

Octahedral

Answer 40

6 electron pairs

90 degrees

Question 41

Square planar

Answer 41

6 electron pairs
4 bonded and 2 lone
90 degrees

Question 42

Pyramidal

Answer 42

4 electron pairs
3 bonded and 1 lone
107 degrees

Question 43

What are Lewis diagrams used to demonstrate?

Answer 43

bonding and non-bonding electrons