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Chem A levels > 1.4 Bonding > Flashcards

1.4 Bonding Flashcards

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1
Q

What is ionic bonding?

A

Elements reacting and gaining/losing electrons

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2
Q

What is covalent bonding?

A

Elements reacting and sharing electrons

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3
Q

You must know how to draw an ionic bond…!

A

Okay

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4
Q

You must know how to draw a covalent bond……!

A

Sure

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5
Q

What causes repulsive forces in an ionic crystal (that stuff bout attraction type shit idk what to say bro)

3 things

A
  • Outershell electrons repelling outershell electrons on neighbouring ion
  • Positive nuclii/nuclei (idk D:) of different ions repelling each other
  • Ions of same charge repel
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6
Q

What determines strength of an ionic bond?

A

Net balance of the attractive and repulsive forces + intermolecular distance between the actions and anions

(i think i’ll stick with net balance¯\__(ツ)__/¯)

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7
Q

Look at yo phone/book for the diagram of a summarisation of forces of attraction and repulsion in an ionic bond

A

Fine

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8
Q

What is a Dative covalent bond?

(coordinate bond)

A

When there’s an extra proton from ig the main metal in the covalent bond?

(so just say an extra proton ig)

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9
Q

What the in depth detail of covalent bonds?

A
  • Electrons shared duhh
  • Spin in opposite directions to overcome natural repulsion between 2 same charge sub atomic particles (wtf)

meh it kinda reminds me of that one other damn question which i never needed to know :(

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10
Q

What defines the attractive force of a covalent bond

A

Electrostatic attraction between negatively charged electron pair + positively charged nuclei of the elements

(gl man buddy o7)

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11
Q

What causes repulsive forces in covalent bond?

A
  • Inner electron shells repelling outer electron shells; in particular the electrons which make up the covalent bond
  • The positively charged nuclei repel each other
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12
Q

Phone/book learn diagram summarising forces of attraction + repulsion in covalent bond

A

Whatever man

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13
Q

How can an ionic compound show covalent properties?

A

Polarisation

Cation attracting electrons on the anion

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14
Q

What 2 ways polarisation can happen

A
  • The bigger and more highly charged anion
  • The smaller and more highly charged cation
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15
Q

Ig i’ll get a picture of both pure ionic and covalent

A

Sigh

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16
Q

Define polar covalent?

A

The electron density distribution is around the anion. The distribution is asymmetrical

17
Q

What is electronegativity?

A

When an atom in a covalent bond attracts the bonding electrons

18
Q

If electronegativity value is less than 0.3 = ?

A

Covalent

19
Q

If electronegativity value is between 0.3 and 1.8 = ?

A

Polar covalent

20
Q

If electronegativity value is greater than 1.8 = ?

A

Ionic

21
Q

What is intramolecular attraction?

A

Occurs within molecules which connects the atoms together

(this force v. strong)

22
Q

What is intermolecular forces?

A

Occurs between molecules to help bind em together

(weaker than intramolecular forces)

23
Q

Explain diamond covalent bond

A
  • Giant covalent (each carbon connected to 4 others by covalent bond)
  • ^ Leads to a high mp (high amount of energy) to overcome
24
Q

Explain methane covalent bond

A
  • Simple covalent (atoms within molecule connected by strong covalent bonds but forces between molecules are weak vdw forces)
  • ^ Very little heat energy needed to overcome = low m and b points
25
Q

Learn diagram representing weak intermolecular forces

A

hawdouhawdohuwad

26
Q

Another word for polar covalent?

A

Permanent dipole

27
Q

Explain the permanent dipole of H-Cl bond

A
  • Cl atom more electronegative than H atom
  • Cl atom pulls e- density towards itself
  • The Cl end becomes more negative than the H end
  • Creating partial charges = a dipole
28
Q

Learn diagram of vdw forces (instantaneous dipole version)

A

Bruhh i’m not sure if i can make it out the hood

29
Q

Quick summary of effects on halogens

A

As u go down the group,
+ electrons,
mp increases,
bp increases,
states change from gas to liquid to solid

30
Q

Dipole effect on solubility explain type shit

A

Simple molecular substances are soluble in non-polar solvents like hexane. This is because the Van der Waals forces form between the simple molecular structure and the non-polar solvent. The formation of these forces weakens the lattice structure.

Fu cking hell just bet this aint in the test buddy ol pal

31
Q

Ima take a picture of this stupid hydrogen bond dipole type shit man

A

Okay, but tbh its basically biology. And guess what? Guess what? GUESS WHAT? I DONT REMEMBER THAT SHIT

32
Q

Why does bp increase as u go down the group 4 of hydrides type shit?

A
  • Molecules getting larger
  • More electrons
  • VDWs dispersion forces become greater
33
Q

How would the bp of alkanes compare to bp of alcohols?

A

Alkanes - Only intermolecular forces are vdw forces (very weak = little heat needed to overcome similarly for bp too)

Alcohols - Only vdw AND hydrogen bonds (which are stronger than vdw so needs more heat energy) ANd also just say how it needs to overcome both forces thats why bp is high

34
Q

Chemical can hydrogen bond = more soluble in water

A small alcohol such as methanol and ethanol is readily soluble in water. But as its carbon chain increases, alcohols become increasingly insoluble. WHY?

A

Methanol and ethanol have short alkyl chains with v. small vdw forces. As chain length increases, the vdw forces between them also increases interfering with the molecules ability to form hydrogen bonds. The alkyl chains are hydrophobic too so its non-polar.

gl man

35
Q

What does VSEPR stand for?

A

V:alence
S:hell
E:lectron
P:air
R:epulsion

36
Q

So these last few pages ima just screenshot it and ye ig it may or may not be ggs but at the end of the day, u tried, idk man hopefully plan A works other plan B is just plan B :(

A

Sigh it may not work bro, expect the unexpected….

Chem A levels (11 decks)

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