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Chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

a chemical bond is

A

a force of attraction

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2
Q

types of bonding

A

metallic, ionic, covalent

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3
Q

bond between a metal and non-metal

A

ionic

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4
Q

bond between a non-metal and another non-metal

A

covalent

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5
Q

bond within a metal

A

metallic

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6
Q

describe an ionic bond

A

metal transfers outer shell electron(s) to the non-metal, so both have a full outer shell - the attraction between positive and negative ions; this attraction is strong

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7
Q

covalent bond

A

non-metals share outer electrons to get a full outer shell

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8
Q

ion

A

electrically charged particles which have a different number of protons and electrons

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9
Q

how positive and negative ions are attracted

A

electrostatic force of attraction - opposite charges attract

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10
Q

empirical formula

A

shows the simplest ratio of atoms in a compound

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11
Q

atom that loses an electron

A

forms a positive ion

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12
Q

atom that gains an electron

A

forms a negative ion

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13
Q

what does the ion charge correspond to

A

group number (for 1=1+ 2=2+ 3=3+ 5=3- 6=2- 7=1-)

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14
Q

pros of the dot cross diagram

A

shows the electron structure of the ions

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15
Q

cons of the dot cross diagram

A

can give the impression that the structure is made of pairs of ions, rather than being a continuous structure containing a massive number of ions

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16
Q

pros of the ball and stick structure

A

helps to show how ions are arranged relative to each other

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17
Q

cons of the ball and stick structure

A

the lines connecting ions may be confused with covalent bonds and it may be though that ions are far apart from each other

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18
Q

pros of the 3D space filling structure

A

gives a very good representation to how ions are packed together

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19
Q

cons of the 3D space filling structure

A

can give the impression that the structure is limited to a few ions rather than being a continuous structure containing a massive number of ions

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20
Q

pros of the 2D space filling structure

A

very easy to draw

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21
Q

cons of the 2D space filling structure

A

only shows the structure in 2D but the lattice is really 3D, can give the impression that the structure is made of pairs of ions, rather than being a continuous structure containing a massive number of ions

22
Q

describe what happens when a lithium atom reacts with a chlorine atom

A

Li transfers 1 outer shell electron to Cl - this gives it a charge of 1+. Cl gains an electron - this gives it a charge of 1-. Both ions now have full valence shells - the opposite charges are electrostatically attracted and form an ionic bond.

23
Q

3 particles found inside an atom

A

proton, neutron, electron

24
Q

particles found in nucleus of an atom

A

neutron, proton

25
Q

in the gold alpha particle experiment, most alpha particles pass straight through gold atoms; why

A

the atoms are not solid - mostly empty space

26
Q

in the gold alpha particle experiment, some alpha particles deflected; why

A

some come into contact with the nucleus which is positively charged, so is deflected - same charges repel

27
Q

two key differences between thomson’s plum pudding model and rutherford’s replacement

A

electrons in fixed orbit - shows protons in nucleus vs being a positive mass

28
Q

atomic number

A

total protons in an atom

29
Q

mass number

A

total protons and neutrons

30
Q

2 structures of covalent bonds are

A

simple molecular structure (AKA covalent molecules e.g. CO2) - Giant molecular structure (AKA giant covalent structure e.g. diamond)

31
Q

many non metal elements exist as

A

simple diatomic molecules that contain covalent bonds

32
Q

how to work out how many covalent bonds a non-metal will make

A

group number - number in outer shell - how many needed to complete - number of bonds

33
Q

metallic bonding

A

atoms in metals - tightly packed in layers - outer electron(s) from each atom is delocalised - is able to move throughout the structure - exist as giant 3D lattices - metal ions and delocalised electrons are attracted by electrostatic forces of attraction - each metal ion is equally attracted to the delocalised electrons

34
Q

properties of ionic substances

A

high melting points - solid at room temperature - do not conduct electricity as solids - conduct electricity when molten or in solution

35
Q

why ionic substances have high melting points

A

strong forces between ions - lots of energy needed to break them

36
Q

why ionic substances only conduct electricity when molten or in solutions

A

as solid, ions in fixed positions and cannot move so cannot carry charge. when molten/dissolved, ions free to move - can carry charge

37
Q

describe structure of ionic compounds when dissolved in water

A

water causes the giant lattices to break apart so ions become individual and are free to move.

38
Q

type of bonding within a molecule

A

covalent

39
Q

intermolecular forces between molecules in simple covalent substances are

A

weak

40
Q

usual state of simple covalent substances

A

gases or liquids

41
Q

boiling points of simple covalent substances

A

low

42
Q

a bigger molecule has what type of IMF and MP

A

stronger intermolecular forces - higher melting point

43
Q

charge of simple covalent substances

A

neutral - dont conduct electricity

44
Q

polymers are what type of molecule

A

very large molecules

45
Q

state of giant covalent substances

A

solids

46
Q

melting points of giant covalent substances

A

very high

47
Q

atomic structure of giant covalent substances

A

all atoms bonded to others by strong covalent bonds which must be overcome to boil/melt these substances

48
Q

molecular formula

A

actual number of atoms

49
Q

allotrope

A

the atoms of the same element are bound to each other in different manners. In other words, the spatial arrangement of atoms is different from one allotrope to another

50
Q

simple vs giant covalent

A

simple - weak IMF between molecules, low M/BP, G/L @RT, molecular formula, relatively small no. atoms, IMF broken in state change, bigger molecules have higher M/BP
giant - high M/BP, S@RT, massive no. atoms, empirical formula, covalent bonds broken in state change

Chemistry (9 decks)

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