Atomic Structure And Electrons (Completed)

Question 1

Define isotopes

Answer 1

Atoms of the same element (so with the same number of protons) with a different number of neutrons

Question 2

What is the mass number

Answer 2

The number of protons + neutrons in the nucleus

Question 3

What is the atomic number

Answer 3

The number of protons in the nucleus

Question 4

Explain how the chemical properties of isotopes differ or are similar

Answer 4

Isotopes have the same chemical properties and react in the same way because they have the same number of electrons - this is what the reactivity mostly depends on

Question 5

Define relative isotopic mass

Answer 5

The mass of an atom of an isotope in comparison with 1/12th of the mass of an atom of carbon 12

Question 6

How can you see the relative isotopic mass of an isotope

Answer 6

The relative isotopic mass is the same as the isotopes mass number

Question 7

Define relative atomic mass

Answer 7

The weighted mean mass of an atom of an element in comparison to 1/12th of the mass of an atom of carbon 12

Question 8

Give 2 things the weighted mean mass of an element takes into place

Answer 8

The percentage Abundance of each isotope

The relative mass of each isotope

Question 9

Give 2 things a mass spectra usually tells us

Answer 9

The number of peaks represents the number of isotopes

The height of the peaks tells us the abundance of the isotope

Question 10

What is the X acis on a mass spectra usually

Answer 10

m/z

Question 11

What does m/z represent

Answer 11

Mass to change ratio

Question 12

What is the max number of electrons in the first shell

Answer 12

2

Question 13

What is the maximum number of electrons in the second shell

Answer 13

8

Question 14

What is the maximum number of electrons in the third shell

Answer 14

18

Question 15

What is the maximum number of electrons in the fourth shell

Answer 15

32

Question 16

Give the 4 different types of orbital

Answer 16

S orbital
P orbital
D orbital
F orbital

Question 17

Define orbital

Answer 17

A region within an atom that can hold up to 2 electrons with opposite spins

Question 18

What is the shape of an s orbital

Answer 18

Spherical

Question 19

How many electrons can occupy s orbitals in each shell

Answer 19

In each shell, a maximum of 2 electrons they can occupy s orbitals

Question 20

What is the shape of a p orbital

Answer 20

The shape of a dumbbell, and there are usually 3 of them which are arranged at right angles to each other

Question 21

How many electrons maximum can occupy a p orbital in each shell

Answer 21

None can occupy a p orbital in the first shell

From shell 2 and up, 6 electrons can occupy a p orbital

Question 22

How many D orbitals can fit in a subshell

Answer 22

5

Question 23

How many electrons can occupy the d Orbitals in each shell

Answer 23

In the first and second shells, no electrons can occupy d Orbitals

From the 3rd shell up, 10 electrons can occupy d Orbitals per shell

Question 24

Draw the table that shows how electrons occupy each shell, sub-shell and orbital

Answer 24

Question 25

What are sub-shells

Answer 25

Groups of the same types of orbital

Question 26

What does the Aufbau principle state

Answer 26

Electrons fill orbitals of the lowest energy first

Question 27

Draw the graph that shows the order each sub shell is filled

Answer 27

Question 28

Give the order that the sub shells are filled in up to 4p⁶

Answer 28

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶

Question 29

What is hund’s rule

Answer 29

Each electron has a negative charge and we would expect the electrons in an orbital to repel one another

Within a sub shell, each orbital has the same energy. Each of the orbitals in a sub-shell has to be filled singly and with parallel spins (same direction) before any electrons can pair up