C3 - The Periodic Table Flashcards Preview

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Flashcards in C3 - The Periodic Table Deck (33)
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0

Who made the first suggestion of the periodic table?

John Dalton

1

How did John Dalton organise the elements?

In order of their masses.

2

How did John Newlands organise the elements?

In order of mass placed in octaves.

3

Why couldn't Newlands concept of the periodic table worked?

He assumed all of the elements had been discovered and the pattern broke down after calcium.

4

How did Mendeleev organise the elements?

In order of their atomic weights then in a periodic pattern.

5

Why did scientists believe Mendeleev's periodic table?

He left space for undiscovered elements and predicted the properties of them. When the elements were discovered his predictions were accurate.

6

How does the atomic number of an element link to the periodic table?

The atomic number determines its position.

7

Hoe does the number of electrons in the outer shell link with the periodic table?

The number of electrons determines its chemical properties and its group number.

8

What two factors connect electronic structure with reactivity going down the groups?

-The distance between the outermost electrons and the nucleus.
-The number of occupied inner shells.

9

Give one limitation of Mendeleev's periodic table.

-Not all elements fit the pattern of ordering by atomic mass.

10

How does reactivity change going down group 1?

Reactivity increases going down.

11

How does reactivity going down group 7?

Reactivity decreases going down the group.

12

Why does reactivity change going down group 1?

The outer electron is easier to lose because the outer shell is further away from the positive nucleus making the attraction weaker.

13

Why does the reactivity change going down group 7?

The electron in the outermost shell is attracted less strongly because it is further away from the nucleus making it harder to attract electrons.

14

What are Group 1 elements known as?

Alkali metals

15

Which elements make up Group 1?

Lithium, Sodium, Potassium, Rubidium, Caesium, Francium

16

Why are Group 1 elements stored in oil?

To prevent them from reacting with oxygen in the air.

17

What is the density of Group 1 metals?

Low compared to other metals.

18

How hard are Group 1 elements?

Very soft, they can be cut with a knife.

19

Why do Group 1 metals turn dull very quickly when cut?

They react with oxygen to form an oxide layer.

20

What type of reaction do Group 1 elements undergo?

Ionic bonding to make 1+ ions.

21

What is the general boiling of Group 1 elements?

The boiling points are low compared to other metals and get lower going down the group.

22

How to Group 1 metals react with water?

Metal + water ----> metal hydroxide + hydrogen

23

What non-metals do alkali metals react vigorously with?

Water and group 7 elements

25

What is produced when group 1 and 7 elements react?

White alkali metal compounds that dissolve in water.

26

What are the properties of transition metals?

- High melting points.
- High densities.
- Strong and hard.
- Good conductors of electricity and energy.
- Relatively unreactive.

27

Why are transition metals useful as structural materials?

They corrode very slowly.

28

What types of compounds do transition metals make?

-Coloured
-Ionic with various charges.

29

What are transition metals useful for?

-Catalysts
-Structural materials

30

What are the properties of Group 7 elements?

-They have low boiling points.
-They are poor conductors of energy.
-They exist as elements in covalent pairs.