Atomic Structure and Other Stuff

Question 1

Proton

Answer 1

Relative charge
+1
R mass
1

Question 2

Neutron

Answer 2

Relative charge
0
Relative mass
1

Question 3

Electron

Answer 3

Relative charge
-1
R mass
1/1840

Question 4

Atomic number

Answer 4

The smaller number next to an element on the periodic table

Atomic no= Number of protons = no of electrons

Question 5

Mass number

Answer 5

Number of particles (protons and neutrons) in the nucleus
Larger number on periodic table
Mass no= no protons + no of neutrons
Mass number - atomic number = no of neutrons

Question 6

Isotope definition

Answer 6

Atoms with the same atomic number but different mass number are isotopes of each other. This means they have the same number of protons but different numbers of neutrons. Same chemical properties because they have the same electronic structures as each other

Question 7

Relative atomic mass

Answer 7

Average value for the relative mass of an atom that takes into account naturally occurring isotopes of the element and their abundances

Question 8

How to calculate the relative atomic mass of an element

Answer 8

(Abundance of isotope x its mass number) + (abundance of other isotope x its mass number) divided by 100 or total of all the abundances

Question 9

Period

Answer 9

Row of elements

Question 10

Group

Answer 10

Column of elements (elements tend to react in a similar way in a group)

Question 11

How to find the electronic configuration of one of first 20 elements

Answer 11

1) find the number of electrons in the atom from its atomic number (smaller number)
2) fill in the shells, remember that the first shell can only hold 2 electrons but the rest hold 8 each
Check by:
The group number of the element is the number of electrons in the outer shell
The period is the number of electron shell