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Chem A levels re-run > OG unit 1.4 > Flashcards

OG unit 1.4 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…!
Do u know how to?

A

Okay
1. Metals try to lose electrons
2. Non-metals try to gain so
3. I mean ye u just draw the gaining and losing
4. Metals = dots
5. Non-metals = crosses

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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 the attractive forces in an ionic crystal?

A

Oppositely charged ions

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6
Q

What causes repulsive forces in an ionic crystal (that stuff bout attraction type shit idk what to say bro) (ima focus on one this, it’s just repulsive forces)

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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7
Q

What determines strength of an ionic bond?

A

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

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

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8
Q

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

He stealin’

A

Fine

The “easy identifiable way” for knowing this:
- U have to of the elements “ionically bonding”
- Arrows between both
- Below and above arrows showing attraction (the black heads coming together)
- Think of it as ionic bonding but “in more detail”

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9
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)

2 electrons deriving from the same atom

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10
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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11
Q

What defines the attractive force of a covalent bond
o7

A

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

(gl man buddy o7)

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12
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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13
Q

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

Sharring

A

Whatever man

Another “easy identifiable way” for knowing this:
- Obviously they are sharing, but looks like dipole type shiii
- There’s a “plus” inside showing repulsion
- North and South have an e-
- East and West have protons, + in a circle, positive ion type shi
- Arrows going to e- or the proton showing attraction

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14
Q

How can an ionic compound show covalent properties?

A

Polarisation

Cation attracting electrons in the anion

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15
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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16
Q

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

(low key, dot and cross diagram)

A

Sigh

17
Q

Define polar covalent?

A
  • When the electron density distribution is around the anion.
  • And the distribution is asymmetrical
18
Q

What is electronegativity?

A

When an atom in a covalent bond attracts the bonding electrons

19
Q

If electronegativity value is less than 0.3 = ?

A

Covalent

20
Q

If electronegativity value is between 0.3 and 1.8 = ?

A

Polar covalent

21
Q

If electronegativity value is greater than 1.8 = ?

A

Ionic

22
Q

What is intramolecular attraction?

A

Occurs within molecules which connects the atoms together

(this force v. strong)

23
Q

What is intermolecular forces?

A

Occurs between molecules to help bind em together

(weaker than intramolecular forces)

24
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
25
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
26
Q

Learn diagram representing weak intermolecular forces

(methane intermolecular forces bro, cmon man)

A

hawdouhawdohuwad

U right, pretty simple, CH4 and the forces between each are weak as hell

27
Q

Another word for polar covalent?

A

Permanent dipole

28
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
29
Q

Learn diagram of vdw forces (instantaneous dipole version)

(halogens from periodic table 1.6 D:)

A

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

If i can learn how to draw this, 1.6 will be a piece of cake brother

30
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

31
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

32
Q

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

Nah bro, this is easy, this is biology water explanation. DONT FAIL ME NOW

A

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

33
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
34
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

35
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

36
Q

What does VSEPR stand for?

A

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

37
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 :(

I’m gonna make another deck exclusively for VSEPR, only when i reach up to here (gl)

A

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

Time is money, i’m not spending my money correctly

Chem A levels re-run (16 decks)

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