10.1- THE HALOGENS Flashcards

1
Q

Is the group 7 elements metals or non-metals?

A

non-metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What do the group 7 elements exist as?

A

diatomic molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the group 7 elements called?

A

halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the appearance of the gaseous halogens?

A

vary in appearance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

At room temperature what colour and state is fluorine?

A

pale yellow gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

At room temperature what colour and state is chlorine?

A

greenish gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

At room temperature what colour and state is bromine?

A

red-brown liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

At room temperatue what colour and state is iodine?

A

black solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Going down group 7 how does the colour and density of the elements change?

A

get darker and denser going down group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What smell does all the halogens have?

A

“swimming-bath” smell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is a number of the properties of fluorine described as?

A

untypical

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Where does many of the untypical properties of fluorine stem from?

A

F-F bond unexpectedly weak, compared with trend for rest of halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the size of fluorine like?

A

small size

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What does the small size of fluorine lead to?

A

repulsion between non-bonding electrons as they’re so close together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

How does electronegativity change going down group 7?

A

decreases going down group 7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How does atomic radius change going down group 7?

A

atomic radius increases going down group 7

17
Q

How does melting point change going down group 7?

A

melting point increases going down group

18
Q

How does boiling point change going down group 7?

A

boiling point increases going down group 7

19
Q

Why does the atoms get bigger going down group 7?

A

because each element has one extra filled main level of electrons compared with one above it

20
Q

What is electronegativity?

A

measure of ability of atom to attract electrons, or electron density, towards itself within a covalent bond

21
Q

What does electronegativity depend on?

A

attraction between nucleus + bonding electrons in outer shell

22
Q

What does the attraction between the nucleus + bonding electrons in the outer shell depend on? (3)

A

depends on balance between number of protons in nucleus (nuclear charge)

distance between nucleus and bonding electrons

shielding effect of inner shells of electrons

23
Q

What happens to the shared electrons in hydrogen halides, HX going down the group?

A

get further away from nucleus as atoms get larger going down group

24
Q

As the shared electrons get further away, what does this mean? (2)

A

shared electrons further from halogen nucleus + increases shielding by more inner shells of electrons

25
Q

Which factors: shared electrons getting further from halogen nucleus + increased shielding OR increasing nuclear charge is more important?

A

shared electrons getting further from halogen nucleus + increased shielding

26
Q

As the shared electrons getting further from the halogen nucleus + increased shielding are the more important factors, what does this mean? (hint-electronegativity)

A

electronegativity decreases going down group

27
Q

Why does melting and boiling point increases going down the group?

A

as larger atoms have more electrons

28
Q

As larger atoms have more electrons how does this affect VDW forces?

A

makes the van der Waals forces between molecules stronger

29
Q

The lower the boiling point the more _____ the element?

A

the more volatile the element