The Periodic Table

Table of Contents

Atomic structure and the periodic table

Review the structure of the sub atomic particles in an atom.
Be able to use the periodic table to determine the structure of an atom
Atomic structure 1. Complete the following table
Sub atomic particle
Charge
mass location Electron
Negative
1/2000 of a proton or neutron
In shells or orbits around the nucleus
Proton
Positive
1
Inside the nucleus
Neutron
None
1
Inside the nucleus

2. What does the atomic number tell us?
The number of protons in an atom defines what element it is. For example carbon atoms have six protons, hydrogen atoms have one, and oxygen atoms have eight.
The number of protons in an atom is referred to as the atomic number of that element. Atomic number is in bottom
3. What does the atomic mass tell us?
The total number of protons and neutrons it contains. The mass number of an atom is never smaller than the atomic number. It can be the same, but is usually bigger.
Mass number at the top
4. Why do most elements in the periodic table have atomic mass that is not a whole number,
The electrons are weighed as well and only play a significant weight amount.

5. Complete the following table
Element

Atomic Number
Atomic mass
Number of protons
Number of electrons
Number of neutrons

C612
6
12
6
6
6

O816
8
16
8
8
8

Fe 2656
26
56
26
26
30

Na1123
11
23
11
11
12

S1632
16
32
16
16
16

Ne1020
10
20
10
10
10

6. What is the plum pudding model of an atom? When was it proposed

The plum model, also known as a blueberry muffin model, of the atom by J.j Thomas was proposes in 1904, the atom is composed of electron surrounded by soup of positive charge to balance the electron’s negative charges , likely negatively charge raisins surrounded by positively charged pudding

7. How is it different from our current idea of an atom?
In Thomas’s view of the atoms of elements consist of a number of negatively

Electron shells

8. What is the octet rule? The first energy level can hold a maximum of two electrons, the second energy level a maximum of eight, and so on.

9. Complete the following table

Nu of electrons in the first shell orbit
Nu of electrons in the 2nd shell orbit
Nu of electrons in the 3rd shell orbit
C612
2
4

O816
2
6

Na1123
2
8
1
S1632
2
8
6
Ne1020
2
8

Periodic table and atomic structure
1. What do all the elements in the same group have in common?
The number of Electrons that have in the outer shell also there properties are similar
2. What do all the elements in the same period have in common?
All elements in the same period have in common is the number of rings they have,
3. Why do you think the lightest elements are near the top of the periodic table and the heaviest are near the bottom?
The lightest elements are near the top because they have less protons and electron it’s going to have a lighter mass.
Elements and the periodic table

Understand what an element is
Be able to identify some of the common elements.
Be aware of how the periodic table of elements developed

Complete the table for the elements on show
Name
Symbol
Description
Metal / non metal /Metalloid
Nickel
Ni
Sliver, bendy, shiny, thin, solid light
Metal
Oxygen
O
Clear, air, gas, non-smell
Non metal
Hydrogen
H
Gas, air, clear
Non metal
Copper
Cu
Bendy, bronze coloured, thin, shiny, sharp, light, solid
Metal
Helium
He
Air, gas, clear
Non metal
Zinc
Zn
Clumps are heavy and non-bendable, sliver, shiny, cold, strips are thin and bendy, light, solid
Metal
Cobalt
Co
Heavy, thick, non- bendable, silver, dull, solid
Metal
Aluminium
Al
Shiny, light, thin, bendable, silver, solid
Metal
Silicon
Si
Looks like tiny rocks, shiny, light, hard, solid
Metalloid