Brainscape's Knowledge GenomeTM

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


See full index

chemistry > bonding > Flashcards

bonding Flashcards

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

what is an ionic bond

A

the ionic bond is the electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion

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

what happens in ionic bonding

A

the metal ion loses an electron and the non mental gain

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

what is an ionic lattice

A

a regular arrangement of alternating positive and negative ions

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

what do the endings -ide and -ate tell you about a substance

A

-ide is a metal reacting with a non-metal forms an -ide compound
-ate is a metal reacting with a non-metal and oxygen to from an -ate compound

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

what particles and forces are present in ionic compounds

A

electrostatic forces of attraction and ions (charged particles)

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

why do ionic compounds have high melting and boiling points

A

they have strong electrostatic forces of attraction which are hard to overcome

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

why do ionic compound only conduct electricity when liquids or dissolved

A

because their ions are free to move from place to place. ionic compounds cannot conduct electricity when solid, as their ions are held in fixed positions and cannot move

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

what is a cation

A

an ion with a positive charge (lost electrons)

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

what is an anion

A

an ion with a negative charge (gained electrons)

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

explain why ionic compounds are usually solid at room temperature

A

strong electrostatic forces
which require a lot of energy to overcome

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

how are covalent bonds formed

A

when pairs of electrons are shared by atoms

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

why do simple molecular compounds have low melting and boiling points

A

very little energy is needed to overcome the intermolecular forces

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

why are simple molecular compounds poor electrical conductors

A

there are no free ions or electrons to carry the charge

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

what is a polymer

A

large molecules made up of repeating chains called monomers

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

how are simple molecular structures different from giant covalent structures

A

simple: have weak intermolecular forces so usually gases or liquids at room temp (low melting and boiling points), dont conduct electricity (no charged particles)

giant: no weak intermolecular forces present between molecules as there are no molecules, only covalent bonds, so substances are solid at room temp, they have high melting and boiling points as they have many strong covalent bonds, most cannot conduct electricity as they do not have free electrons nor charged particles

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

what are allotropes

A

different forms of the same element with different structures

17
Q

what are some allotropes of carbon

A

diamond, graphite

18
Q

explain the differences in structure between the different allotropes of carbon

A

diamond- each C atom has 4 covalent bonds
graphite- each C atom has 3 covalent bonds

19
Q

what are the properties of diamond and graphite

A

diamond- doesnt conduct electricity as there are no free moving charges. has a high melting point because a large amount of energy is needed to overcome the many strong covalent bonds

graphite- does conduct electricity as there are delocalised electrons that are free to move between layers of graphite. high melting points due to strong covalent bonds

20
Q

what are the uses of diamond and graphite

A

diamond- very hard so used for cutting tools and jewellery
graphite- used as a lubricant as the layers can slide over each other

21
Q

what are fullerenes

A

molecules of carbon arranged inclosed tubes /hollow balls

22
Q

how are particles arranged in metals

A

the metal atoms are arranged in a regular pattern of layers, with delocalised electrons able to move between them

23
Q

what are the properties of metals in terms of bonding

A

high melting and boiling points- there are strong electrostatic forces of attraction between the positive metal ions and the negative delocalised electrons which require a lot of energy to break

good conductors of heat and electricity- the delocalised electrons are free to move and carry a charge through the whole structure

malleable- arranged in layers which slide over each other when force is applied~

24
Q

what does malleable mean

A

can be bent without breaking

chemistry (5 decks)

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