Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > 3.1.3 Bonding > Flashcards

3.1.3 Bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is ionic bonding?

A

The electrostatic force of attraction between oppositely charged ions in a lattice.

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

What is the formula for a sulfate ion?

A

SO4^2-

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

What is the formula for a hydroxide ion?

A

OH-

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

What is the formula for a nitrate ion

A

NO3^-

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

What is the formula of a carbonate ion?

A

CO3^2-

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

What is the formula for an ammonium ion?

A

NH4^+

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

What are the 4 crystal structures?

A

Ionic
Metallic
Molecular
Macromolecular

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

What is the definition of a single covalent bond?

A

A shared pair of electrons.
(Multiple bonds contain multiple pairs of electrons)

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

What is the definition of a co-ordinate bond?

A

It contains a shared pair of electrons with both electrons supplied by one atom.

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

What is the definition of metallic bonding?

A

The electrostatic attraction between delocalised electrons and positive ions arranged in a lattice.

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

What are some examples of crystal structures?

A

Diamond
Graphite
Ice
Iodine
Magnesium
Sodium chloride

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

What are the physical properties of ionic structures?

A

-They conduct electricity when molten or dissolved- the ions in the liquid are free to move.
-High melting points- they have a lattice structure so there are strong electrostatic forces which require lots of energy to overcome.
-Tend to dissolve in water- water molecules are polar, the charged particles pull ions away from the lattice.

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

What is the definition of a macromolecular structure?

A

A huge network of covalently bonded atoms.

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

What are the physical properties of graphite?

A

-Lubricant- there are weak bonds between layers which are broken easily so, the sheets can slide over each other.
-Electrical conductor- there are delocalised electrons which are free to move through the sheet.
-Low density- the layers are far apart so, it’s used for strong lightweight sports equipment.
-High melting point- strong covalent bonds.
-Insoluble- covalent bonds are too strong.

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

What are the physical properties of diamond?

A

-Tetrahedral shape
-High melting point
-Hard
-Good thermal conductor- vibrations travel easily through the lattice
-Bad electrical conductor- Outer electrons are in localised bonds
-Insoluble
-Used for gemstones as it refracts light a lot

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

What are the physical properties of metallic structures?

A

-Good conductors- sea of delocalised electrons to carry flow of charge.
-Malleable- the layer of positive Ions can slide over each other. The delocalised electrons prevent fragmentation as they move around the lattice.
-High melting point/solid at room temp- strong electrostatic attraction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What are the physical properties of molecular structures?

A

-Consist of covalently bonded molecules held together by weak Ven der Waals forces.
-Low melting and boiling points- Not much energy required to overcome van der waals forces.
-Poor conductors- no charged particles.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Which factors affect the strength of a metallic bond?

A

Charge on the metal ion
Ionic radius
Number of delocalised electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What factors affect the strength of ionic bonding?

A

Ionic radius
Charges on ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Why are specific bond angles formed?

A

Pairs of electrons in the outer shell arrange themselves as far apart as possible to minimise repulsion. Bonding pairs and lone pairs are clouds of charge that repel each other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Which types of repulsion are the strongest?

A

Lone pair-lone pair > lone pair-bond pair > bond pair-bond pair

22
Q

What is the effect of lone pair repulsion on the bond angle?

A

It reduces it by 2.5 degrees

23
Q

What is electronegativity?

A

The power on an atom to attract the bonding electron pair towards itself within a covalent bond.

24
Q

Which factors affect electronegativity?

A

Size
Nuclear charge

25
Q

What happens to electronegativity across a period?

A

It increases because the atomic radius decreases, due to increasing nuclear charge and similar shielding.

26
Q

What happens to electronegativity down a group?

A

It decreases as shielding increases.

27
Q

What is a polar bond?

A

A bond formed between 2 atoms with different electronegativities. (Electron distribution is unsymmetrical, and a permanent dipole may form.)

28
Q

Why do some molecules with polar bonds not have a dipole?

A

The charge distribution is symmetrical so, charges cancel out

29
Q

What causes a permanent dipole?

A

A difference in charge causing a difference in electron density.

30
Q

What is an induced dipole?

A

Forms when the electron orbitals around a molecule are influenced by another charged particle.

31
Q

What is a quick method to figure out if a bond is polar or not?

A

If it has different terminal atoms or if the central atom has a lone pair, the molecule is likely to be polar.

32
Q

What determines molecule shape?

A

The number of electron pair
If they’re bonding or lone pairs.

33
Q

What types of electron pairs and bond angle is present in a V- shaped molecule?

A

2 bonding pairs
2 lone pairs
104.5

34
Q

What types of electron pairs and bond angle is present in a trigonal planar molecule?

A

3 bonding pairs
120

35
Q

What types of electron pairs and bond angle is present in a trigonal pyramidal molecule?

A

3 bonding pairs
1 lone pair
107

36
Q

What types of electron pairs and bond angle is present in a tetrahedral molecule?

A

4 bonding pairs
109.5

37
Q

What types of electron pairs and bond angles are present in a trigonal bipyramid molecule?

A

5 bonding pairs
90 and 120

38
Q

What types of electron pairs and bond angle is present in a octahedral molecule?

A

6 bonding pairs
90

39
Q

What types of electron pairs and bond angle is present in a seesaw molecule?

A

4 bonding pairs
1 lone pair
90 and 120

40
Q

What types of electron pairs and bond angle is present in a T- shaped molecule?

A

3 bonding pairs
2 lone pairs
90 and 180

41
Q

What types of electron pairs and bond angle is present in a square planar molecule?

A

4 bonding pairs
2 lone pairs
90

42
Q

What are the 3 types of intermolecular forces?

A

Van der Waals
Permanent dipole-dipole
Hydrogen bonds

43
Q

Which properties are influenced by intermolecular forces?

A

Melting and boiling points

44
Q

What is a van der waals force?

A

Induced dipole attraction

45
Q

How does atomic radius affect Van der Waals forces?

A

The larger the molecules, the more electrons and mass it has. So, the forces are stronger.

46
Q

What is a permanent dipole-dipole force?

A

The force of electrostatic attraction between two polar molecules.

47
Q

How are hydrogen bonds formed?

A

H is really small and becomes very positive when bonded to F, O or N as they have high electronegativities. The bonds are always linear.

48
Q

Which type of intermolecular force is the strongest?

A

Hydrogen bond > permanent dipole-dipole > Van der Waals
But Van der Waals can be stronger depending on the size of the molecule.

49
Q

How does shape affect Van der Waals forces?

A

The more long or straight a molecule is, the closer the two molecules can get increasing the strength of the bond.

50
Q

Why does water expand as it turns into ice?

A

As liquid water cools to form ice, the molecules make more hydrogen bonds and arrange themselves into a regular lattice structure.
In this regular structure the molecules are further apart on average than the molecules in liquid water - so ice is less dense than liquid water.

Chemistry (14 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions