1.2 b Bonding relating to properties Flashcards Preview

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Flashcards in 1.2 b Bonding relating to properties Deck (36)
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1

Why do elements take part in reactions?

To achieve a full outer shell

To achieve a stable electron arrangement

To achieve a noble gas electron arrangement

2

What is a covalent bond?

A shared pair of electrons

3

What type of elements form covalent bonds?

 

( LO : 18 )

Noin - metal elements

4

What holds the atoms together when they form covalent bonds?

( LO : 17 )

The common (electrostatic) attraction the nuclei have for the shared pair of electrons.

 

5

How do non-metal atoms achieve a full outer shell when they react with one another?

They share unpaired electrons

6

Why do elements take part in reactions?

( L.O.19)

To achieve a full outer shell and achieve a noble gas electron arrangement.

7

How do non-metal atoms achieve a full outer shell when they react with one another?

( L.O.19)

They share unpaired electrons

8

What are the 7 elements that exist as diatomic molecules?

( L.O. 20)

9

What is meant by a diatomic molecule?

( L.O. 20)

 

 

A molecule made up of 2 atoms

10

What 4 shapes of molecules must we know?

( L.O 21)

11

What are the properties of covalent molecular substances?

( L.O. 24)

12

Why do covalent molecular substances have low melting and boiling points?

( L.O.  24)

13

Why do covalent network substances have high melting and boiling points?

14

What are the properties of covalent network substances?

15

What is a molecule?

16

Are covalent molecular substances soluble in any other liquids?

Yes. Hexane for example

17

What is an ion?

An atom which has lost or gained electron(s)

18

What kind of elements take part in ionic bonding?

Metals reacting with non-metals

19

Why do metals lose electrons to form positive ions?

To obtain a full outer shell

20

How many electrons do metals lose to form ions?

The number of valence electrons that they have.

 

e.g  Na loses 1

        Mg loses 2

21

What charge do metal ions have when they lose electrons?

They take on the corresponding positive charge as the number of electrons they lose.

 

e.g Mg loses 2 electrons to become Mg2+

22

Why do non-metals form negative ions?

They gain electrons (-1 charge) to complete their outer shell.

23

Why is water a "polar" molecule?

24

Why are many ionic compounds soluble in water?

25

Why do ionic substances conduct in solution but not in solid state?

The ions are free to move in solution but are trapped in the lattice in the solid

26

Why do ionic compunds have high melting points?

27

Do ionic substances conduct in

 

  1. Solid state
  2. Solution
  3. Liquid state

  1. No
  2. Yes
  3. Yes

28

Recognising an ionic lattice

( LO 32)

29

What is meant by a lattice?

A regular, repeating, 3-D structure.

30

What is electrolysis?

The breaking apart of an ionic substance using electricity

31

What type of current is used in electrolysis and why?

DC current

To ensure separate products form at each electrode

32

What happens at the negative electrode during electrolysis?

Reduction of metal ions into metal atoms.

Reduction is gain of electrons

33

What happens at the positive electrode during electrolysis?

Oxidation

Negative ions lose electrons to form atoms (usually as molecules)

34

Do ionic compounds have low or high melting points?

(LO 33)

High

35

Why are many ionic compounds soluble in water?

( LO 34 )

Polar water molecules are able to attract the ions and break the lattice

36

What is the conductivity of ionic substances?

( LO 35)