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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

When 2 different ______ join together, you get a compound.

A

elements

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2
Q

______ bonding is when ions are held together by electrostatic attraction

A

ionic

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3
Q

________ attraction holds positive and negative ions together - it is very strong

A

electrostatic

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4
Q

The overall charge of any compound is ________

A

zero

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5
Q

Magnesium chloride contains Mg2+ and Cl- ions

What would the balanced formula be for this

A

MgCl2

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6
Q

Sodium chloride is an example of a _____ _____ _______ structure

A

giant ionic lattice

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7
Q

Ionic compounds conduct electricity when…

A

they are molten or dissolved as there are free electrons and ions are free to move

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8
Q

Ionic compounds have _____ melting points

A

high because they are held together by strong electrostatic forces which needs a lot of energy to overcome.

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9
Q

Ionic compounds tend to _______ in water

A

dissolve as water is polar and the charged parts pull ions away from the lattice causing it to dissolve.

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10
Q

What type of bond holds molecules together?

A

strong covalent bonds

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11
Q

What does a single covalent bond share?

A

a pair of electrons

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12
Q

Covalent bonding happens between 2 _____________

A

non metals

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13
Q

Carbon atoms can form what type of structure due to them forming 4 strong covalent bonds?

A

giant covalent structure

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14
Q

How are the carbon atoms arranged in graphite?

A

sheets of flat hexagons covalently bonded with 3 bonds each. the fourth outer electron of each carbon atom is delocalised

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15
Q

Give examples of the properties of graphite

A
  • weak bonds between the layers so easily broken so sheets can slide over eachother
  • delocalised electron carry a charge so graphite is an electrical conductor
  • low density so can be used to make strong lightwewight equipment
  • high melting point due to strong bonds

-insoluble in any solvent

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16
Q

In diamond, each carbon atom is covalently bonded to ____ other carbon atoms and arrange themselves in a _________ shape

A

4

tetrahedral

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17
Q

Give examples of the properties of diamond

A
  • very high melting point
  • hard
  • good thermal conductor
  • cant conduct electricity as all electrons are held in localised bonds
  • wont dissolve in any solvent
  • can be cut
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18
Q

define dative covalent bond and what is it represented by

A

dative covalent bond is where both electrons come from one atom

represented by an arrow pointing away from the donor atom

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19
Q

electron charge clouds repel each other, give order of repulsion from highest to lowest

A

lone to lone
lone to bonding
bonding to bonding

20
Q

how to work out how many electron pairs a shape has?

A

take the central atom
work out how many electrons in outer shell
add one to this number for every atom it is bonded to
divide by 2 to find number of electron pairs
compare electron pairs to number of bonds to find the number of lone pairs and bonding pairs

21
Q

shapes with 2 electron pairs

A

linear - no lp

22
Q

shapes with 3 electron pairs

A

trigonal planar - no lp

23
Q

shapes with 4 electron pairs

A

tetrahedral - no lp
trigonal pyramidal - 1 lp
v shaped - 2 lp

24
Q

shapes with 5 electron pairs

A

trigonal bipyramidal - no lp
seesaw - 1 lp
t shaped - 2 lp

25
Q

shapes with 6 electron pairs

A

octahedral - no lp
square planar - 2 lp

26
Q

define electronegativity

A

an atoms ability to attract the electron pair in a covalent bond

27
Q

which element is most electronegative ?

A

fluorine

28
Q

in a covalent bond between two atoms of different electronegativities, the bonding electrons will be pulled toward the more electronegative atom. this makes the bond ____

A

polar

29
Q

In a polar bond, the difference in electronegativity between the two atoms causes a permanent _____

A

dipole

30
Q

Define dipole

A

a difference in charge between the two atoms caused by a shift in electron density in the bond

31
Q

What happens to a bond when electronegativity increases?

A

becomes more polar

32
Q

In a substance made up of molecules that have permanent dipoles, there will be weak ________________ _____ of attraction between + and - charges on neighbouring molecules

A

electrostatic forces

33
Q

Where are Van der Waals forces found?

A

between all atoms and molecules

34
Q

How are VDW created?

A

Electrons in charge clouds are moving really quickly. At any moment the electrons in an atom are more likely to be at one side - this would create a temporary dipole. The dipole can cause another temporary dipole in the neighbouring atom/ other direction. They are then attracted to each other.

35
Q

In a solid at room temperature, what forces are holding them together in a lattice?

A

Van der Waals

36
Q

What is the strongest type of intermolecular force?

A

Hydrogen bonding

37
Q

rule for hydrogen bonding?

A

H bonds with N, O, F

38
Q

Examples of molecules with hydrogen bonding

A

water and ammonia

39
Q

properties of substances with hydrogen bonding

A

higher bp and mp
more energy needed to break bonds

40
Q

why is ice less dene than liquid water?

A

As liquid water cools to form ice, the molecules make more H bonds and arrange into a regular lattice structure.
In this, the H2O molecules are further apart on average than molecules in liquid water so ice is less dense.

41
Q

Metals exist as giant metallic lattice structures and have a _________ ______ ‘sea’

A

delocalised electron

42
Q

describe metallic bonding

A

The + metal ions are attracted to the delocalised - electrons. They form a lattice of closely packed positive ions in a sea of delocalised electrons.

43
Q

properties of metals

A

high mp due to electrostatic attraction
the more there are, the stronger the bonding so higher mp

good thermal conductors as the delocalised electrons can pass kinetic energy to eachother

good electrical conductors because the delocalised electrons can move and carry a charge

metals are insoluble because the strength of the metallic bonds

44
Q

What do you need to overcome to melt or boil a simple covalent compound?

A

intermolecular forces

you dont need to break the much stronger covalent bonds that hold the atoms together - this is why simple covalent compounds have relatively low mp and bp

45
Q

A substance will only conduct electricity if it contains ______ particles that are ____ to move.

A

charged

free

46
Q

As water is a polar solvent, what type of particles dissolve well?

A

polar or charged

Chemistry (10 decks)

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