M2 - Atomic Structure & Electron Structure

Question 1

What is the shape of a p-orbital?

Answer 1

Dumbbell / figure eight

Question 2

Explain the rule of orbitals filling in order of increasing energy

Answer 2

1s is filled first.
For n=2 shell, filling order is: 2s, 2p
For n=3 shell, filling order is 3s, 3p, 3d

Question 3

Explain the rule of orbitals with the same energy are occupied singly first

Answer 3

Within a sub shell, the orbitals have the same energy. One electron occupies each orbital before pairing begins. This prevents repulsion until no unoccupied orbitals remain.

Question 4

Explain why isotopes have the same chemical properties (1)

Answer 4

Same number of electrons in the outer shell / same electron configuration

Question 5

What can an electron be thought of as?

Answer 5

A negative-charge cloud with the shape of the orbital, called an electron cloud.

Question 6

What happens in terms of energy sub-shells when forming ions?

Answer 6

The highest energy sub-shells lose or gain electrons.

Question 7

What are the rules of orbital fillings?

Answer 7

Orbitals fill in order of increasing energy.
Electrons pair with opposite spins.
Orbitals with the same energy are occupied singly first.

Question 8

Do isotopes react differently?

Answer 8

No, because chemical reactions involve electrons, not neutrons.

Question 9

How can electron configuration be shortened?

Answer 9

1s2 can be expressed as [He].
1s2 2s2 2p6 can be expressed as [Ne].
1s2 2s2 2p6 3s2 3p6 can be expressed as [Ar].

Question 10

What charge does a neutron have?

Answer 10

0

It is neutral

Question 11

What is the charge of an electron?

Answer 11

-1

Question 12

What does atomic number represent?

Answer 12

The number of protons.

Question 13

How could the fraction of the isotopes of carbon be found experimentally in the lab? (1)

Answer 13

Mass spectrometry

Question 14

What is relative atomic mass?

Answer 14

The weighted mean mass of an atom of an element relative to 1/12th of the mass of an atom of carbon-12.

Question 15

Explain the rule of electrons pair with opposite spins

Answer 15

Electrons are negatively charged and repel one another.
Electrons can have spin up or spin down.
If electrons have opposite spin, the charge repulsion is counteracted enough for both to be in the orbital.

Question 16

What are shells made up of?

Answer 16

Subshells and Atomic orbitals

Question 17

Define relative isotopic mass (2)

Answer 17

Mass of the isotope compared to 1/12th of the mass of a carbon 12

Question 18

What is the shape of an s-orbital?

Answer 18

Spherical

Question 19

Shells are also regarded as what?

Answer 19

Energy levels

Question 20

How many orbitals does each type contain?

Answer 20

S - one
P - three
D - five
F - seven

Question 21

What happens to energy as the shell number increases?

Answer 21

Energy increases

Question 22

What are isotopes?

Answer 22

Atoms of the same element with the same number of protons but with different numbers of neutrons.

Question 23

How are electrons arranged?

Answer 23

In shells around the nucleus

Question 24

Where does the electrons filling subshells in energy level order rule cause confusion?

Answer 24

The 3d sub-shell has higher energy than the 4s.

So the 4s fills before the 3d.

Question 25

What are the different sub shells? How many orbitals and electrons do they have?

Answer 25

S-subshell- 1 orbital - 2 electrons
P-subshell- 3 orbitals- 6 electrons
D-subshell- 5 orbitals- 10 electrons
F-orbitals- 7 orbitals- 14 electrons

Question 26

Answer 26

B

Question 27

Answer 27

55%

Question 28

Answer 28

1s subhell =2
3p orbital = 2
third shell = 18

Question 29

What makes up the nucleus?

Answer 29

Protons and neutrons

Question 30

What subatomic particle occupies the region around the nucleus?

Answer 30

Electrons

Question 31

Answer 31

Question 32

Why do atoms have no overall charge?

Answer 32

The same number of electrons and protons so the charges cancel out.

Question 33

How many electrons can be held in an orbital?

Answer 33

One or two, no more.

Question 34

What is the shell number referred to as?

Answer 34

Principal quantum number

Question 35

Answer 35

A

Question 36

What is relative isotopic mass?

Answer 36

The weighted mean mass of an isotope relative to 1/12th of the mass of an atom of carbon-12.

Question 37

Define relative atomic mass (3)

Answer 37

The weighted mean mass of an atom relative to 1/12th the mass of one atom of carbon 12

Question 38

What does mass number represent?

Answer 38

The number of protons and neutrons.

Question 39

Define isotopes (1)

Answer 39

Atoms of an element with the same number of protons but a different number of neutrons

Question 40

How many electrons can be held in each orbital type?

Answer 40

S - two
P - six
D - ten
F - fourteen

Question 41

What is the charge of a proton?

Answer 41

+1

Question 42

How are percentage abundances of the isotopes in a sample of an element found?

Answer 42

Experimentally using a mass spectrometer.

Question 43

What is the electron configuration for Chromium (Cr)? (1)

Answer 43

1s2 2s2 2p6 3s2 3p6 4s1 3d5

Question 44

What is the electron configuration of Copper (Cu)? (1)

Answer 44

1s2 2s2 2p6 3s2 3p6 4s1 3d10