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Chem Mock > Bonding > Flashcards

Bonding Flashcards

1
Q

What is ionic bonding

A

transfer of electrons from a metallic element to a non-metallic element to form a full outer shell

electrostatic attraction formed between the oppositely charged ions

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2
Q

Cations and anions

A

Forming cations by the removal of electrons from metals
Forming anions by the addition of electrons to nonmetals

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3
Q

what are ionic compounds

A

Cations and anions are oppositely charged and therefore attracted to each other
Electrostatic attractions are formed between the oppositely charged ions to form ionic compounds

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4
Q

melting points in ionic

A

high melting points

attraction is very strong and requires a lot of energy to overcome

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5
Q

why are ionic lattice neutral

A

Ions in a lattice are arranged in a regular repeating pattern so that positive charges cancel out negative charges

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6
Q

when does ionic radius increase/decrease

A

Ionic radii increase with increasing negative charge
Ionic radii decrease with increasing positive charge

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7
Q

how does the strength of ionic bonding depend on charge

A

ionic charge. Bigger charges exert greater attractive forces between each other so the greater the charge on the ions involved, the stronger an ionic bond will be.

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8
Q

how does the strength of ionic bonding depend on ionic radius

A

he smaller the ions, the more closely they can be packed together in the ionic lattice. The shorter the distance between oppositely charged ions, the stronger the electrostatic forces between them and hence the stronger the ionic bond.

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9
Q

why does ionic radius increase a group

A

This is because as we go down a group, the number of outer electron shells increases.

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10
Q

why does ionic radius decrease along a period

A

Nuclear charge increases as more protons. Therefore, electrons are pulled in more strongly.

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11
Q

what are isoelectronic ions

A

the same electronic configuration but different numbers of protons, therefore will have a different ionic radius

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12
Q

how does the radius of isoelectronic ions work

A

As the number of protons in the nucleus of the ion increases, the electrons get pulled in more closely to the nucleus
The radii of the isoelectronic ions therefore fall across this series of ions

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13
Q

when can ionic compounds conduct electricity

A

conduct electricity when molten or dissolved because only then are the ions of the compound able to move and carry charge. Ionic compounds are unable to conduct electricity when solid because the ions are fixed in place and unable to carry charge.

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14
Q

why are ionic compounds soluble in water

A

ionic compounds and water molecules are partially charged molecules (polar). This means the partial charges of water break apart the ionic lattice, pulling oppositely charged ions apart and the ionic compound to dissolve

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15
Q

what are ionic compounds arranged in

A

giant ionic lattices.

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16
Q

what does it mean if ionic compounds are solids

A

there isn’t enough energy to overcome the strong electrostatic forces of attraction between the oppositely charged ions that make up the lattice
Therefore, high temperatures are required to make an ionic compound melt or boil

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17
Q

what does the solubility of ionic compounds depend on

A

Breaking down the ionic lattice
The polar molecules attracting and surrounding the ions

18
Q

what is the evidence for existence of ions

A

electrolysis is a clear piece of evidence for the existence of ions
Positive ions in solution are attracted to the negative electrode
Negative ions in solution are attracted to the positive electrode
CuCrO4
Cu2+ ions (blue)
CrO42- ions (yellow)
blue colour appears around the negative electrode, and a yellow colour appears around the positive electrode

19
Q

what is a covalent bond

A

electrostatic attraction between nuclei of two non-metal atoms and the bonding electrons

20
Q

What us dative covalent bonding

A

Some molecules have a lone pair of electrons that can be donated to form a bond with an electron-deficient atom

21
Q

what is bond energy

A

energy required to break one mole of a particular covalent bond in the gaseous states

22
Q

what is bond length

A

internuclear distance of two covalently bonded atoms

23
Q

when does bond length decrease

A

The greater the forces of attraction between electrons and nuclei, the more the atoms are pulled closer to each other
This decreases the bond length of a molecule and increases the strength of the covalent bond

Triple bonds are the shortest and strongest covalent bonds due to the large electron density between the nuclei of the two atoms
This increase the forces of attraction between the electrons and nuclei of the atoms
As a result of this, the atoms are pulled closer together causing a shorter bond length
The increased forces of attraction also means that the covalent bond is stronger

24
Q

What are the bonding pair, lone pair and bond angle of linear

A

bonding - 2
lone - 0
bonding angle - 180

25
Q

What are the bonding pair, lone pair and bond angle of v-shaped

A

bonding - 2
lone - 2
bonding angle - 104.5

26
Q

What are the bonding pair, lone pair and bond angle of trigonal planar

A

bonding - 3
lone pair - 0
bonding angle - 120

27
Q

What are the bonding pair, lone pair and bond angle of triangular pyramid

A

bonding - 3
lone pair - 1
bonding angle - 107

28
Q

What are the bonding pair, lone pair and bond angle of tetrahedral

A

bonding - 4
lone pair - 0
angle - 109.5

29
Q

What are the bonding pair, lone pair and bond angle of trigonal bypyramidal

A

bonding - 5
lond - 0
angle - 90 and 120

30
Q

What are the bonding pair, lone pair and bond angle of octahedral

A

bonding - 6
lone - 0
angle - 90

31
Q

describe metallic bonding

A

lattice of positive ions / regular arrangement of positive ions
(1)
(in sea of) delocalised electrons
(1)
strong forces of attraction between ions and delocalised electrons (so high melting temperature)
(1)
so lots of (heat) energy needed to break attraction between ions and delocalised electrons / metallic bonds

32
Q

state conditions when magnesium bromide conducts electricity

A

molten and dissolved in water

33
Q

predict two physical properties of a metal

A

high melting/ boiling temperature

strong (electrostatic) attraction between metal ions and delocalised electrons

  • (good) electrical conductivity/ thermal conductivity
  • mobile delocalised electrons (1)
  • malleability/ ductility

*the layers of ions/ atoms can easily slide over each other

34
Q

what is a covalent bond

A

(strong electrostatic) attraction
(1)
between two nuclei and the share /bonding pair of electrons

35
Q

what does giant structure suggest

A

therefore contains many strong covalent bonds

36
Q

why does co2 have polar bonds but its not a polar molecule

A

carbon dioxide is a symmetrical/linear molecule and so the dipole moments/vectors cancel

37
Q

why is H20 polar molecule

A

oxygen is more electronegative than hydrogen

(M2) which results in a polar bond with oxygen delta negative so hydrogen delta positive

38
Q

why do dipole moments of water no cancel

A

lone pairs of electrons of oxygen mean that the dipole moments vectors do not cancel

39
Q

what things do you need to make reference to when talking about difference in boiling temperatures

A

London forces
which has more electrons
where dipole dipole is stronger
electronegativity
ALL TYPES OF DIFFERENT BONDS

40
Q

how is london forces formed

A

uneven distribution of electrons results in formation of instantaneous dipole in first molecule which induces second dipole on another molecule

41
Q

why does hydrogen bonding cause ice to be less dense than liquid water

A

as hydrogen bonds are longer than covalent bonds

more open / more space between molecules (making it less dense)
(1)
* due to (3 Dimensional) lattice / ring structure in ice (1)

42
Q

three things

A

Chem Mock (34 decks)

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