2.1.1

Question 1

What are the masses and charges of the subatomic particles?

What are their positions in the atom?

Answer 1

Electron orbits the nucleus in energy levels/shells, charge -1, mass 1/2000
-protons and neutrons in nucleus, both have a mass of 1, charge of +1 on proton, charge of 0 on neutron.

Question 2

What do atoms have to have(in terms of subatomic particles) and why?

Answer 2

Same number of protons and electrons as they have to be neutral(have no overall charge).

Question 3

The number of protons determines the?

Why cant this be different for the same element?

Answer 3

Element,

If protons change element is different.

Question 4

The number of electrons determines the?

Answer 4

Chemical properties.

Question 5

What do the relative atomic mass and the atomic number show on the periodic table?
How can these be used to work out the number of subatomic particles in ions, isotopes and atoms?

Answer 5

In a atom:
-protons, atomic number
-electrons, same as atomic number
-neutrons, relative atomic mass-atomic number
In an ion:
-protons, atomic number
-electrons if negative add charge number to atomic number, if positive minus charge number from atomic number
-neutrons, relative atomic mass-atomic number
In an isotope:
-protons, atomic number
-electrons, same as atomic number
-neutrons, relative atomic mass-atomic number.

Question 6

What is the role of neutrons?

Answer 6

Acts as a glue preventing the positive protons in the nucleus repelling each other.

Question 7

What is an isotope?

Answer 7

Same number of protons and electrons, different number of neutrons.

Question 8

What is the relative atomic mass?

Answer 8

The weighted mean mass of an atom compared to mass of 1/12th of a carbon 12 atoms mass.

Question 9

What is relative isotopic mass?

Answer 9

The mass of an isotope compared to 1/12th of a carbon 12 atoms mass.

Question 10

How is relative molecular mass worked out and when is it used?
What is a simple molecule?

Answer 10

The RAM of each atom in the molecule is added,
used for molecules,
simple molecule(2+ atoms bonded covalently.

Question 11

When the can the relative molecular mass not be used and what is used instead?
How do you work this out?

Answer 11

Relative molecular mass cannot be used for giant ionic or giant covalent compounds, as molecules must have a fixed number of atoms,
add all the RAM of each atom of the formula unit.

Question 12

How to work out RAM?

Answer 12

{(mass x abundance)+(mass x abundance)}
/total abundance

if percentages are used put them in to the abundance and use 100 for the total abundance.

Question 13

Why is the word relative used?

Answer 13

Protons and neutrons have relatively the same mass so 1/12 of carbon 12 can be used as one unit or the atomic mass unit.

Question 14

What can mass spectrometry tell us?

Answer 14

• a unknown element
• the relative atomic masses or the relative isotopic masses
• the abundance of isotopes.`

Question 15

How does a mass spectrometer work(basic overview)?

Answer 15

The sample is bombarded with electrons by an electron gun, this knocks out an electron from the isotopes(giving them a +1 charge, the ions are measured by the mas spectrometer.

Question 16

What does the mass spectrometer measure specifically and why is the fact that the isotope becomes an ion not important in this measurement?

Answer 16

The mass:charge(mass to charge ratio) is measured, electrons have a negligible mass so the loss of an electron doesn’t affect the mass of the isotope.

Question 17

What is the mass:charge ratio equivalent to?

Answer 17

The relative isotopic mass of an isotope.