1Atoms are made up of which particles?
Protons, neutrons, and electrons
2What charge does an electron have?
-1 charge
3Where do electrons move around in an atom?
In orbitals around the nucleus
4What part of the atom takes up most of its volume?
The orbitals
5Where is most of the mass of an atom concentrated?
In the nucleus
6How does the size of the nucleus compare to the whole atom?
The nucleus is very small compared to the entire atom
7What particles are found in the nucleus?
Protons and neutrons
8Why are relative mass and charge used for subatomic particles?
Because their actual mass and charge are very small
9What is the relative mass and charge of a proton?
Relative mass = 1, Relative charge = +1
10What is the relative mass and charge of a neutron?
Relative mass = 1, Relative charge = 0
11What is the relative mass and charge of an electron?
Relative mass = 1/2000, Relative charge = -1
12What does a nuclear symbol show?
The number of subatomic particles
13How do you calculate the number of neutrons from a nuclear symbol?
Subtract the bottom number from the top number
14What differs between ions and neutral atoms?
Ions have different numbers of protons and electrons
15How are ions formed?
Atoms lose or gain electrons
16Do negative ions have more protons or more electrons?
More electrons than protons
17What are isotopes?
Atoms of the same element with different numbers of neutrons
18Do isotopes have the same number of protons?
Yes, they have the same number of protons
19What decides the chemical properties of an element?
The number and arrangement of electrons
20Why do isotopes have the same chemical properties?
They have the same electron configuration
21How do the physical properties of isotopes differ?
Isotopes have different densities, rates of diffusion, etc., due to different masses