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Chemistry C2 > C2.2 > Flashcards

C2.2 Flashcards

(58 cards)

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1
Q

periods

A

horizontal rows

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2
Q

groups

A

vertical columns

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3
Q

who created the periodic table?

A

Mendeleev

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4
Q

ions

A

charged particles that have either lost or gained electrons

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5
Q

ionic bonding

A

metal + non-metal

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6
Q

covalent bonding

A

non-metal + non-metal

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7
Q

describe covalent bonding

A

-when non metal atoms react, they need to gain electrons to fill their outer shell
-they can only do this if they share their electrons

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8
Q

what are strong covalent bonds a result of?

A

electrostatic attraction between positive nuclei of the atoms and the pairs of negative electrons that are shared between them

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9
Q

properties of simple covalent bonds

A

-2 or more non metals
-mostly gases
-low melting and boiling points
-don’t conduct electricity
-low density

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10
Q

why do covalent molecules have a low density?

A

molecules are not closely packed together

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11
Q

why do covalent molecules have low melting and boiling points?

A

strong covalent bonds are not what is broken apart it is the weak intermolecular forces between the bonds that is broken

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12
Q

why do covalent molecules have a low conductivity?

A

there must be free moving charged particles to conduct electricity and covalent molecule have no free moving ions

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13
Q

metal properties

A

-malleable
-shiny
-sonorous
-conducts electricity and heat
-solid at room temperature
-ductile
-high density

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14
Q

non-metal properties

A

-not shiny
-brittle
-doesn’t conduct electricity or heat
-variety of states at room temperature
-low density

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15
Q

differences between the old and new periodic table

A

-fewer elements
-no atomic numbers
-gaps

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16
Q

describe ionic bonding

A

during a chemical reaction between a metal and a non-metal, the reacting atoms either lose or gain electrons to achieve a full outer shell

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17
Q

metal ions

A

lose electrons and form cations

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18
Q

non-metal ions

A

gain electrons and form anions

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19
Q

structure of ionic compounds

A

-oppositely charged ions are arranged in a regular way to form a giant ionic lattice

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20
Q

what do giant ionic lattices result in?

A

the formation of crystals

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21
Q

what is the overall net charge of an ionic compound?

A

it has no overall net charge

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22
Q

properties of ionic compounds

A

-high melting and boiling points
-conducts electricity when molten or in a solution
-crystalline and brittle
-soluble in water

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23
Q

why do ionic compounds have high melting and boiling points?

A

the strong ionic bonds must be broken which requires a lot of energy

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24
Q

why do ionic compounds only conduct electricity when molten?

Study These Flashcards
A

in a solid the ions aren’t free to move, in a solution they are free to move and you need freely moving particles to hold a charge

25
why are ionic compounds crystalline and brittle?
when you put pressure on the compound, ions who have the same charge come next t each other and repel, causing it to shatter
26
why are ionic compounds soluble in water?
chloride ions are attracted to the hydrogen ions, the sodium ions are attracted to the oxygen ions and the compounds are separated by the water molecules because of the oppositely charged attraction
27
malleable
capable of being hammered or pressed into shape without breaking or snapping
28
ductile
capable of being drawn into thin wires without breaking
29
metallic bonds
metal + metal
30
describe metallic bonds
strong electrostatic attraction between delocalised electrons and positive metal ions
31
what are the properties of metallic bonds?
-high melting and boiling points -good conductors -flexible
32
why do metallic bonds have high melting and boiling points?
they have very strong metallic bonds which require a lot of energy to break
33
why are metallic bonds good conductors?
delocalised electrons are free to move and carry a charge
34
why are metal bonds flexible?
the layers can slide over each other which is why they are malleable and ductile
35
alloy
mixture of two or more metals
36
allotropes
different forms of the same element that have different properties because their atoms are arranged differently
37
properties of giant covalent structures
-very high melting and boiling points -crystalline appearance -hard -generally don't conduct electricity -insoluble in water
38
why do covalent structures have high melting and boiling points?
consists of very strong bonds which require a lot of energy to break
39
why do covalent structures have a crystalline appearance?
ordered in a giant lattice structure
40
why are covalent structures hard?
made of rigid covalent bonds
41
why do covalent structures generally not conduct electricity?
every carbon atom is bonded to other carbon atoms so there are no delocalised electrons left over
42
comparing metals with alloys
metal: has regular layers which means they can slide over each other when stretched or bent alloys: don't have regular layers as the different type of metal distorts the layers which makes it harder for layers to slide over each other
43
what are giant covalent structures?
consists of millions of non-metal atoms joined by covalent bonds and arranged in a repeating regular pattern
44
what are the different abilities of carbon?
-forms four chemical bonds to other atoms -bond itself forming long straight, branched and even ring carbon chains -form single, double or even triple bonds
45
describe the structure of graphite
-made from repeating hexagons that form layers or sheets -this leaves each carbon with a 'spare' electron that isn't used in bonding, these spare electrons are free to move between the layers -this means carbon is bonded to three other carbon atoms
46
what is an example of a giant covalent structure?
silicone dioxide
47
what are fullerenes used for?
lubricants
48
polymers
very long covalent molecules
49
LDPE
low density polyethene e.g. plastic bags
50
HDPE
high density polyethene e.g. hard hat
51
increasing the chain length of polymers
-long polymer chains have stronger intermolecular forces than shorter ones -by making the chains of polymers longer, a stronger and less flexible material is produced with a higher melting point
52
modifying polymers using cross linking
-addition of cross links between polymers makes the material tougher, less flexible and increases melting point -crosslinks are chemical bonds that links polymer chains together
53
thermosoftening polymer
gets softer when heated
54
thermosetting polymer
gets harder when heated
55
limitations to the particle model
-scale of nucleus to the electrons is wrong in most models -models show bonds as physical structures -most models do not give an accurate idea of the 3D shape of a molecule -bond lengths are not in proportion to the size of the atom
56
what are synthetic polymers commonly called?
plastic
57
what is an example of a naturally occurring polymer?
silk
58
how do polymers form?
when lots of small covalent molecules called monomers join together

Chemistry C2 (3 decks)

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