2. Atomic Structure

Question 1

Where is the proton found in the atom, what is its relative mass and charge?

Answer 1

nucleus, 1, +1

Question 2

Where is the neutron found in the atom, what is its relative mass and charge?

Answer 2

Nucleus, 1, 0

Question 3

Where is the electron found in the atom, what is its relative mass and charge?

Answer 3

Shells, 1/1840, -1

Question 4

How can we calculate % abundance of an isotope?

Answer 4

(Amount of isotope/total amount of all isotopes) x 100

Question 5

How can we calculate RAM using abundance?

Answer 5

Σ(Mass of isotope x relative abundance) / Σ relative abundance

Question 6

how do mass spectra?

Answer 6

• molecule enters mass spectrometer and is vaporised then ionised by collision with a beam of high energy electrons
  M(g) + e- > M+(g) + 2e-
• M+ has the same RMM as the parent molecule M
• number of peaks = number of isotopes

Question 7

Describe the shape of the s sub shell

Answer 7

Circular

Question 8

Describe the shape of the p sub shell

Answer 8

Figure of eight

Question 9

What is the max number of electrons in the s subshell?

Answer 9

2

Question 10

What is the max number of electrons in the p subshell?

Answer 10

6

Question 11

What is the max number of electrons in the d subshell?

Answer 11

10

Question 12

What is the max number of electrons in the f subshell?

Answer 12

14

Question 13

How many orbitals are there in the s subshell?

Answer 13

1

Question 14

How many orbitals are there in the p subshell?

Answer 14

3

Question 15

How many orbitals are there in the d subshell?

Answer 15

5

Question 16

How many orbitals are there in the f subshell?

Answer 16

7

Question 17

Which subshell is at an unusual energy level below another subshell?

Answer 17

4s subshell is at a lower energy level than a 3d subshell

Question 18

Define principal quantum number

Answer 18

n, a number representing the overall energy of each orbital. It increases with distance from the nucleus

Question 19

Define shell

Answer 19

A group of atomic orbitals with the same quantum number, n

Question 20

Define atomic orbital

Answer 20

A region within the atom that can hold up to two electrons with opposite spins. It’s a region of space where there’s a 95% chance of finding an electron

Question 21

Define ground state

Answer 21

An electronic configuration in which all the electrons are in the lowest available energy levels

Question 22

What is the aufbau principle?

Answer 22

• Used to determine the ground state electronic configuration
• electrons are placed in unfilled orbitals in the lowest available energy level
• max 2 electrons can share the same orbital, spinning in opposite directions
• if several orbitals of equal energy are available they are first occupied singly before pairing up. This minimises repulsion

Question 23

What are the two exceptions to the Aufbau principle?

Answer 23

Cu = ... 3d10 4s1
Cr = ...3d5 4s1

Question 24

Define first ionisation energy and give the equation to represent it

Answer 24

The energy requires to convert one mole of gaseous atoms into gaseous ions with a single positive charge
X (g) > X+(g) + e-

Question 25

Define second ionisation energy and give the equation to represent it

Answer 25

The energy required to convert one mole of gaseous ions with a single positive charge into gaseous ions with a double positive charge X+(g) > X2+(g) + e-

Question 26

Define third ionisation energy and give the equation to represent it

Answer 26

The energy required to convert one mole of gaseous ions with a double positive change into gaseous ions with a triple positive charge X2+(g) > X3+(g) + e-

Question 27

What variables can affect ionisation energy?

Answer 27

Nuclear charge Electron shielding Distance (Stability of filled and half filled sub shells)