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Grade 11 Chemistry > Exam Review > Flashcards

Exam Review Flashcards

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1
Q

what are the strong bases?

A

NaOH, KOH, LiOH, Ca(OH)2, Ba(OH)2, Mg(OH)2 (alkaline and alkaline earth metals)

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2
Q

what are the strong acids

A

all halogens except for fluorine (Cl, Br, I), HNO3, H2SO4, HClO3, HClO4.

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3
Q

ni=nf, therefore? (this one is to make u feel smart)

A

CiVi=CfVf

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4
Q

how to do concentration calculations?

A
  1. turn the % to grams

2. X given volume (in ml)

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5
Q

what is concentration?

A

amount of stuff in a unit of space.

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6
Q

what affects solubility

A

molecular size, temp, and pressure.

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7
Q

solubility in ionic compounds

A

ion-dipole attractions - for substance to dissolve, the water must have a stronger attraction to ions than that they have to themselves

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8
Q

how does solubility do in covalent compounds

A

polar dissolves polar.

dipole dipole attractions form quite strong inter molecular forces, hydrogen bonding is even stronger bonds.

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9
Q

how strong are solute-solute attractions when the solute dissolves

A

not as strong as the solute-solvent attractions

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10
Q

why is water a universal solvent?

A

water molecules are small, they are highly polar, and they form hydrogen bonds

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11
Q

how to find ions from a solution stoich

A
  1. balanced equation and volume to L
  2. mole ratio to find LR
  3. find amount of element with ionic equation
  4. c=n/v
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12
Q

how to find the mass of a precipitate stoich

A
  1. volume to L
  2. concentration of both known X volume to find mols
  3. find limiting reactant and mols of unknown
  4. times mols by molar mass to find mass
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13
Q

how to do titration stoich

A
  1. volume to L
  2. write out balanced chemical equation
  3. concentration known X volume known for mols known
  4. mol ratio for mols unknown
  5. mol divided by volume for concentration unknown
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14
Q

how does metal reactivity change from acids to bases?

A

it doesnt change, both react with metal.

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15
Q

how does conductivity change from acid to base

A

it doesnt change, both are conductive

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16
Q

how does the colour of phenothalein change from acid to base

A

acids are colourless, bases are magenta

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17
Q

how does feel change from acid to base

A

acids have no characteristic feel, bases are slippery

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18
Q

how does taste change from acid to base

A

acids are sour bases are bitter

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19
Q

what is the law of partial pressures?

A

Ptot= Pa+Pb…

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20
Q

what is the combined gas law?

A

P1V1/T1 = P2V2/T2

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21
Q

what is the ideal gas law?

A

PV=nRT

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22
Q

what is % yield

A

actual/theoretical

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23
Q

what is the EF rhyme?

A

% to mass
mass to mole
divide by small
multiply til whole

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24
Q

how to do good ol stoich? with one known, one unknown, and no concentration crap

A

mass to moles, mole to mole using ratio, to other mass.

25
Q

what is required for combustion?

A

fuel, oxygen, and heat.

26
Q

what are the products of a complete combustion?

A

co2 and h2o

27
Q

whats an ionic compound?

A

a metal with a nonmetal

28
Q

what is a covalent compound?

A

a metal and metal or two nonmetals

29
Q

how do bond dipoles work?

A

its an arrow, pointing to the more elcetronegative atom.

30
Q

what affects periodic trends?

A

size, ionization energy, electronegativity, and electron affinity

31
Q

how does atomic radius change throughout the periodic trends

A 
Increases vertically, as more valence shells are added gong down each period
Decreases horizontally (left to right) because of the increase of protons and electrons, protons are stronger, so when they’re added to the nucleus they pull their electrons closer from the far out valence shell.
32
Q

how does ionization energy effect peroidic trends

A

As the valence ring gets filled with more electrons and the nucleus gets more protons that attract said electrons, the likelihood of the atom to lose electrons decreases. As the rings get further away from the nucleus they get more likely to be lost.
TL;DR ionization energy increases going left to right, and decreases going down

33
Q

how does electronegativity change on periodic table

A

Number of the negative charges increase, causing the positive charged, lonely ions to swoop in.
Summary- increases left to right, decreases going down.

34
Q

how does electron affinity change on periodic table?

A

increases (becomes more negative) left to right

decreases going down.

35
Q

how to name ionic compounds?

A

metal 1st, nonmetal 2nd, change end to ‘ide’

36
Q

how to calculate AAM

A

Mass 1 X frequency 1 + mass 2 X frequency 2 +…

37
Q

how does effective nuclear charge change through the periodic table?

A

it grows moving down the period, causing the atom size to get pregressively smaller

38
Q

what happens to oxianions (ie PO₄³⁻) when an oxygen is added?

A

“per” prefix is added, keeps “ate” suffix

39
Q

what happens to oxianions (ie PO₄³⁻) when an oxygen is removed?

A

no prefix, “ate” suffix gets changed to “ite”

40
Q

what happens to oxianions (ie PO₄³⁻) when two oxygens are removed?

A

prefix gets changed to “hypo”, suffix gets changed to “ite”

41
Q

what happens to acids (ie H₃PO₄) when an oxygen is added?

A

prefix of “per” is added, “ic” suffix stays the same

42
Q

what happens to acids (ie H₃PO₄) when an oxygen is removed?

A

no prefix, suffix changes to “ous”

43
Q

what happens to acids (ie H₃PO₄) when two oxygens are removed?

A

prefix of “hypo”, suffix of “ous”

44
Q

what is an acid salt?

A

metal + hydrogen + polyatomic

45
Q

how to name with “ous”/”ic” thing

A

ous = lower cation charge
ic = higher cation charge
write anion with “ide” ending

46
Q

how to name and identify covalent compounds

A

nonmetal and nonmetal

name with prefixes (fun!)

47
Q

what is dispersion force?

A

the only type of intermolecular force that can be formed by non-polar molecules. it increases with the size of the molecule and surface area.

48
Q

what are the signs of a chemical reaction

A

gas bubbles produced, precipitate, heat, irreversible

49
Q

what is the lil graphic thingy for stoic-like questions

A

things n < XM - /M> m

hope that makes sense

50
Q

what are the diatomic elements?

A

fluorine, chlorine, bromine, iodine, nitrogen, oxygen, and hydrogen

51
Q

hope we dont have to do this… but how do you draw a bohr-rutherford diagram?

A

1st shell only holds 2 electrons, inside nucleus has protons and neutrons

52
Q

how does dissociation go?

A

split up the aqueous products, make a really long reaction that hs all products all nicely listed out and balanced

53
Q

how to draw lewis dot structures?

A

count the valance electrons, place the least electronegative atom in the middle, rarely oxygen, and never hydrogen. distribute so that u have all full shells (unless otherwise stated)

54
Q

what are conjugate acid base pairs?

A

two substances that differ by a single proton.

55
Q

what is the arrhenius theory

A

acids and bases dissolve in water to form oh- and h+ ions.

56
Q

why is water the best?

A

it is highly polar its small, and its basic when pure.

57
Q

what is an ideal gas compared to real gasses?

A

ideal gasses act perfectly, they move in straight lines and are weightless, whereas real gasses ruin everyone’s expectations.

58
Q

hope that helps!

A

if you have mastered the deck (congrats!) but dont feel like youre going to master the exam (shucks!) you can study other decks in this class.

59
Q

what is ionization energy?

A

the amount of energy required to move a valance electron.

Grade 11 Chemistry (5 decks)

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