Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Bonding, Structures and Nano Particles > Flashcards

Bonding, Structures and Nano Particles 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 an Ion

A

Charged Particle Formed when an atom loses or gains electron

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

Define Cation

A

Positive ion

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

Define Anion

A

Negative Atom

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

What is a Molecular Ion

A

Charged particle containing more than one atom

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

Describe Ionic Bonding

A

involves attraction between oppositely charged ions

Ionic bonds are very strong and require a large substantial amount of energy to break them

Typical of Metal Compounds

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

What is a single covalent bonds

A

A shared pair of electrons

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

What is a Molecule

A

two or more atoms covalently bonded

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

What does diatomic mean

A

Two more more atoms covalently bonded

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

Strength of Covalent Bonds

A

Very Strong
Require Large amount of energy to break covalent bond

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

Explain Metallic bonding

A

Results from the attraction between positive ions in a regular lattice and the delocalized electrons

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

What is a lattice

A

Regular arrangement of particles in three dimensions

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

What are delocalized Electrons

A

Delocalized Electrons are the outer shell electrons in the metal which are free to move through the structure

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

How do Ionic Compounds exists when they are solids

A

ionic lattice(alternative positive and negative ions in all directions)

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

What is an Ionic Lattice

A

alternate positive and negative ions in a regular arrangement

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

Properties of Ionic Compoundd

A

High Melting and boiling points(strong and require large amounts of energy to break it)

Cannot conduct electricity as solid(ions cannot move and carry charge)

Can conduct electricity when DISSOLVED IN WATER(Ions can move and carry charge)

Soluble in water

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

What are Van der Waal Forced

A

Weak intermolecular Forces between Covalent molecules

16
Q

Properties of Molecular Covalent Substances

A

Low Melting Points and Boiling points(exist as gases, liquids and Van Der Waals forces are weak)

Cannot conduct Electricity(do not have charged Particles)

Soluble in water

17
Q

Examples of Giant Covalent Structures

A

Diamond
Graphite
Graphene

18
Q

Define Allotrope

A

Different Forms of Same lement

19
Q

Arrangement of Diamond

A

Each Carbon Atom is Covalently Bonded to 4 other Carbon Atoms

20
Q

Arrangement of Graphite

A

Each Carbon Atom is Covalently bonded to 3 other Carbon Atoms

21
Q

Arrangement of graphene

A

Single layer of Graphite

22
Q

Properties of Diamond

A

Does not conduct electricity(does not contain free ions)

Hard(Strong Covalent Bonds and rigid 3d structure)

High Melting and Boiling point(Many strong covalent bonds, require large amount of energy to break them)

23
Q

Properties of Graphite

A

Conduct electicty(Contains delocalised electrons which can carry and move charge)

Soft(Weak bonds between layers(see diagram))

High Melting and Boiling Points(many strong covalent bonds and require large amount of energy to break them)

24
Q

Properties of Graphene

A

Conduct electricity(Contains delocalized electrons which can carry and move charge)

Strong(Many strong covalent bonds)

High Melting and Boiling Points(many strong covalent bonds and require large amount of energy to break them)

25
Q

Use of Diamond

A

Cutting tools(hard)

26
Q

Use of Graphite

A

Pencils

Layers can slide over each other and off to a piece of paper when used it pencil

27
Q

Use of Graphene

A

Batteries as it can conduct electricity

28
Q

Properties of Metallic Structure

A

Conduct Electricity(delocalized electrons )

High Melting/boiling points(Strong covalent bonds)

Malleable(positive Ions can slide over each other without disrupting the bonding)

Ductile(positive Ions can slide over each other without disrupting the bonding

29
Q

Define Alloy

A

Mixture of elements, at least
one of which is a metal, and the resulting mixture has
metallic properties;

30
Q

Define Nanoparticles

A

Structures that are 1-100 nanometers in size,

contain a few hundred atoms

31
Q

Benifits of Nano Particles

A

Nanoparticles are used in sun creams as they give better skin coverage, rub on clear and give
better protection from the ultraviolet rays from the Sun

32
Q

Risks of Nano Particles

A

They may cause cell damage and as they wash off from our skin,
they may be harmful for the environment.

Chemistry (6 decks)

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