Atomic Structure

Question 1

What is the structure of an atom?

Question 2

What is the relative mass and charge of protons?

Question 3

What is the relative mass and charge of neutrons?

Question 4

What is the relative mass and charge of electrons?

Question 5

What is the mass number?

Question 6

What is the atomic number?

Question 7

Why do atoms have an overall neutral charge?

Question 8

Why do atoms of the same element have the same chemical properties?

Question 9

What are ions?

Question 10

What are isotopes?

Question 11

Why do isotopes of the same element have the same chemical properties but different physical properties?

Question 12

What is relative atomic mass?

Answer 12

The average mass of an atom of an element compared to 1/12th of the mass of an atom of carbon-12.

Question 13

What is relative isotopic mass?

Answer 13

The average mass of an atom of an isotope compared to 1/12th of the mass of an atom of carbon-12.

Question 14

What is the equation to calculate the relative atomic mass?

Question 15

What is the relative molecular mass ( Mr)?

Answer 15

The average mass of a molecule compared to 1/12th of the mass of an atom of carbon-12.

Question 16

What does a mass spectometer do?

Answer 16

It shows you the relative atomic mass of an element or the relative abundance of its isotopes.

Question 17

What are the steps to mass spectroscopy?

Answer 17

1. Ionisation.
2. Acceleration.
3. Ion drift.
4. Detection.

Question 18

What happens during ionisation?

Question 19

What happens during acceleration?

Answer 19

The ions are accelerated by an electric field and the same amount of kinetic energy is applied to each ion. The lighter ions will accelerate more.

Question 20

What happens during ion drift?

Question 21

What happens during detection?

Question 22

How many orbitals and electrons does an s-subshell have?

Question 23

How many orbitals and electrons does an p-subshell have?

Question 24

How many orbitals and electrons does an d-subshell have?

Question 25

How many orbitals and electrons does an f-subshell have?

Question 26

What are the rules for figuring out the electronic configuration?

Answer 26

1. Electrons fill up higher energy levels first. 2. Electrons fill up orbitals singly first and then they pair up. 3. An electron is removed from the highest energy level first.

Question 27

What is the different about the electronic configuration of transition metals like cooper and chromium?

Answer 27

1. They only have one electron in the 4s subshell. 2. When they become ions they lose electrons from their 4s subshell before their 3d subshell.

Question 28

What is the electronic configuration for chromium?

Question 29

What is the electronic configuration for cooper?

Question 30

What is the electronic configuration for Fe 2+?

Question 31

What is the first ionization energy?

Answer 31

The energy needed to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions.

Question 32

What factors affect ionisation energy?

Answer 32

1. Nuclear charge. 2. Distance from the nucleus. 3. Shielding

Question 33

What is the second ionisation energy?

Question 34

Why are second ionisation energies higher compared to first ionisation energies?

Question 35

What is the trend in ionization energies as you go down group 2?

Question 36

What is the trend in ionization energies as you go across period 3?

Question 37

What are the exceptions to this rule in period 3?

Question 38

How can you use successive ionisation energies to figure out how many shells an atom has?