History Of Periodic Table

Question 1

Properties of Mendeleevs table

Answer 1

All elements arranged in atomic mass
Left gaps so he could predic what the properties the undicvoverd elements would have

Question 2

How did the atom change over time

Answer 2

John dalton thought they were tiny spheres that couldn’t be divided

Thompson discoed electrons and made the plupudding model

Rutherford held alpha particle test on plum pudding day most radi went through and figured out atoms have concentrated ball of mass at nucleas and that it’s possibly charged

Neil’s Bohr discovered that atoms orbit the nucleas on energy shells
And Chadwick discovered neutrons

Question 3

What is the formula for a buckmister fullerene

Answer 3

C60

Question 4

Properties of nanotubes

Answer 4

Have high tensile strength and resist being stretched
Can be added in sports equipment to make them stronger

Question 5

How are Bucky balls used

Answer 5

To carry drugs into the body
It’s a corny structure

Question 6

What are the conversions of dm and cm

Answer 6

1 dm to 1000cm

Question 7

How do you cslutlate concentration

Answer 7

Mass (g)
———/
Vol(dm)

Question 8

Why do the halogens decrease in deacoty as you go down the group

Answer 8

The atomic mass of the halogens increases

They increase in electron shells
So their atoms are larger as you go down the group
Therefore the attraction od the putter electrons decrease

Question 9

Why do more reactive halogens displace wah other

Answer 9

More reactive halogens atoms oxidise the less reactive halide atoms

Question 10

Properties of metallic bonding

Answer 10

Electrostatic attraction between potitive metal ions and delocalised electrons
The organiseation of electrons and metal ions give metals properties such as malleability and abutting to conduct electricity

Question 11

Why are nano particles better than larger molecule

Answer 11

Cheaper and more efficant

Question 12

What’s the mass mole and mr triangle

Answer 12

Mass
——————
Mr x mole

Question 13

Properties of diamond and graphite.

Answer 13

Diamond
Forms 4 covealnt bonds
Hardest structure on earth due to rigid structure
Dosnt conduct electricity due to doloclaised electrons
Very high melting and boiling point sude to strong electrostatic forces

Graphite
Forms 3 covalent bonds
Soft and slippery due to layers sliding over each other
Conducts electcity due to each atom having 1 delocalised electrons
Melting and boiling point isn’t as high as diamond due to the electrostatic forces not being as strong