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Grade 11 Exam Reviews > SCH3U Exam Review > Flashcards

SCH3U Exam Review Flashcards

1
Q

Precision vs Accuracy

A

Precision: How close something is to the other shots, tries etc.

Accuracy: How close something is to the target.

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2
Q

Determining the amount of sig-digs

A

Significant digits are:

  • Non-zeros Ex, 1-9
  • Zeros between two non-zeros Ex, 109
  • Zeros after a decimal place Ex, 32.0

Significant digits are NOT:

  • Zeros before any other non-zero Ex, 0.000042
  • Zeros ending a number without a decimal Ex, 95300

*Least amount of sig-digs is always used in answers

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3
Q

5 Clues a Chemical Reaction has taken place

A
  • Colour change
  • Odour change
  • Bubbles
  • Precipitate
  • Heat or light is produced
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4
Q

Particle Theory

A

All matter consists of many, very small particles which are in a continual state of motion

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5
Q

Metals and Non-Metals on the Periodic Table

A

Metals:

  • left side and central part of periodic table
  • solids
  • lustrous
  • good conductors
  • high melting points
  • many are flexible, ductile and malleable

Non-Metals:

  • right side of periodic table
  • mostly gasses and powdery solids
  • not shiny, ductile or malleable
  • low melting points
  • only liquid is bromine
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6
Q

Chemical families (Groups) on the Periodic Table

A

Vertical Columns:
Alkali Metals - Far left Column 1 shiny, soft, highly reactive with water and air
Alkali Earth Metals - Column 2 shiny and will burn bright colours
Noble Gasses - Far right Column 8 colourless, odourless, tasteless and very stable
Halogens - Column 7 very reactive, many are poisonous

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7
Q

Trends in the Periodic Table:

Orbits and Valence Electrons

A

Orbits: Elements have the same number of orbits as the number of the period they are in.

Valence Electrons: Elements have the same number of valence electrons as the number of the group they are in.

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8
Q

Trends in the Periodic Table:

Atomic Radius, Ionization Energy, Electron Affinity and Electronegativity

A

Atomic Radius: Increases down and to the left

Ionization Energy: Increases up and to the right

Electron Affinity: Increases up and to the right

Electronegativity: Increases up and to the right

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9
Q

What is an isotope?

A

An isotope is an atom of the same element that has different number of neutrons

Ex, /Users/CaitSforza/Desktop/Screen Shot 2016-01-25 at 10.43.15 AM.png

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10
Q

What is the difference between an ionic compound, polar molecular compound and non-polar molecular compound?

A

Ionic compound: Metal and a Non-Metal 1.67-3.3EN

Polar molecular compound: 2 Non-Metals 0.5-1.67EN

Non-Polar molecular compound: 2 Non-Metals 0-0.5EN

To find/predict EN for a compound take EN of each element and subtract

*EN=Electronegativity

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11
Q

Naming Compounds:

Ionic Compounds:
Molecular Compounds:
Acids:
Binary Acid:

A

Ionic Compounds: Non-metals change ending to -ide
Ex, Silver Iodide

Molecular Compounds: Add correct prefix for number of atoms for each element
Ex, Dinitrogen Monoxide

Acids: Ending changes from -ate to -ic or -ite to -ous
Ex, Sulphuric Acid or Nitrous Acid

Binary Acid: Add prefix hydro- and suffix -ic
Ex, Hydrochloric Acid

*Include bracketed numbers for Cu, Fe, Pb and Sn
Ex, Copper(II)

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12
Q

Assigning states to all reactants and products in a chemical equation

A

Metals: Solids (Except Mercury is liquid)

Non-Metals: Gasses or powdery solids (Except Bromine is liquid)

Metalloids: Mostly Solids

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13
Q

Predicting products between a metal oxide and water and a non-metal oxide and water

A

A metal oxide and a water always create a base

A non-metal oxide and water always create an acid

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14
Q

Predicting products for the decomposition of binary compounds, metal carbonates, metal nitrates and metal hydroxides

A

Binary Compound: Breaks down into elements

Metal Carbonates: Break down into a metal oxide and carbon dioxide gas

Metal Nitrates: Break down into a metal nitrite and oxygen gas

Metal Hydroxides: Break down into a metal oxide and water

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15
Q

Identify complete and incomplete combustion reactions and predict products for each

A

Complete Combustion: Sufficient oxygen is present (Blue flame)
Hydrocarbon + Oxygen = Carbon Dioxide + Water

Incomplete Combustion: Insufficient oxygen is present (Yellow flame)
Hydrocarbon + Oxygen = Carbon Dioxide + Water + Carbon Monoxide + Carbon

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16
Q

Identify a neutralization reaction and predict the products or reactants of a neutralization reaction.

A

Acid + Base = Ionic Salt + Water (Double Displacement)

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17
Q

Predict the products of a double displacement reaction that forms water or a gas (carbon dioxide or ammonia)

A

Forms a Water: Neutralization (Acid + Base = Ionic Salt + Water)

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18
Q

What is a mole? Why is it used by chemists?

A

A mole is the base unit that is used to measure the amount of a substance. Chemists use it because atoms are too small too count and see and they work with large quantities of them.

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19
Q

Avogadro’s number

A

6.02×10^(23) Atoms, Molecules or Formula Units (f.u.)

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20
Q

The difference between atoms, formula units and molecules when using avogadro’s number

A

Atoms (used with a singular element) Ex, Fe(s)
Molecules (used with non-metals) Ex, H2O(l)
Formula Units (used with metal+non-metal) Ex, NaCl(s)

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21
Q

Calculating the percent composition of a substance using formula or from mass data

A 
Unknown Formula (Mass Data): 
total mass of element in compound/total mass of compound x100

With Formula:
M of element in compound/M of compound x100

22
Q

Finding the empirical formula of a substance from the percent composition or from mass data

A

Shows the smallest whole number ratio

  • Assume 100g
  • Find # of mol (Divide by M)
  • Find ratio (Divide by smallest mol #)
23
Q

Finding the molecular formula of a substance from percent composition or from mass data

A

Shows the number of atoms

molecular M given number/Empirical M=# you multiply the empirical ratio by

24
Q

Determing the amount of excess reactant left over when a reaction is complete

A

excess moles = initial moles - moles used

*moles used = LR mole ratio to XS moles

25
Q

Unsaturated vs saturated vs supersaturated solutions

A

Unsaturated: A solution that could dissolve more solute

Saturated: A solution that could not dissolve more solute

Supersaturated: A solution that has more solute than it can dissolve

26
Q

Factors that affect the rate of dissolving and explanations at the molecular level

A
  • Temperature Increases = Rate of Dissolving Increases because particles are moving faster and colliding more often
  • Agitation/mixing Increases = Rate of Dissolving Increases because particles are being forces to come in contact with the undissolved particles at a higher rate
  • Particle Size Decreases = Rate of Dissolving Increases because it causes the surface are to increase creating more exposure to the solvent
27
Q

Types of intermolecular forces and their role in solubility of substances

A

Dipole-Dipole Forces: Intermolecular attraction between two polar molecules

Ion-Dipole Bonds: Intermolecular attraction between ions and polar molecules. Very weak making solubility easy

Hydrogen Bonds: Intermolecular attraction between hydrogen atoms and very electronegative atoms (H-O, H-S, H-N, H-F) Very strong bond, solubility is difficult/impossible

28
Q

Finding the molar concentration of solutions and ions

A

C=n/V

29
Q

Preparing solutions and dilutions-calculations

A

C1V1=C2V2, C=n/V

30
Q

Writing ionic equations and net ionic equations

A

Ionic Equation: Each element set individually with its charge, state and its coefficient (solids cannot separate)

Net Ionic Equation: Only the elements that form a reaction in the equation (The precipitate)

*make sure precipitate will form before writing out equation

31
Q

Acid properties and examples

A

Sour, conductive, corrodes tissues and metals, creates hydrogen gas, turns litmus paper red, colourless in phenolphthalein, pH of 0-7

32
Q

The pH scale and acid-base colour indicators

A

0-7: Acid (red)
7: Neutral
7-14: Base (blue)

33
Q

Properties of strong acids vs weak acids at molecular level and examples

A 
Strong Acids:
HBr - Hydrobromic Acid
HCl - Hydrochloric Acid
HI - Hydroiodic Acid
HNO - Nitric Acid
H2SO4 - Sulfuric Acid

Strong Bases:
Any metal + OH (except Beryllium)

34
Q

Determining if an acid or base is strong or weak

A

Acid:

  • High concentration of ions
  • Completely ionizes in water

Base:
-Based of the degree of the dissociation in water

35
Q

States of matter and predicting the state of a substance based on the type of intermolecular forces present

A

Solid: Strong forces between particles

Liquid: Weak forces between particles

Gas: Very Weak forces between particles

36
Q

Properties of Solids, Liquids and Gases

A

Solid: Fixed volume, fixed shape, strong forces between particles, incompressible, vibrational motion of molecules

Liquid: Fixed volume, variable shape, weak forces between particles, incompressible, vibrational, rotational and translational motion of molecules

Gas: Variable volume, variable shape, very weak forces between particles, compressible, vibrational, rotational and translational motion of molecules

37
Q

Physical properties of Gases

A
  • Gasses are compressible
  • Gasses expand as temperature increases
  • Gasses have very low viscosity
  • Gasses have very low densities
  • Gases are miscible (able to mix completely with each other)
38
Q

Ideal Gas

A

No volume and no attractive forces between particles

39
Q

Kinetic Molecular Theory

A
  • Gas particles are in constant, random motion
  • Gas particles don’t create forces between one another
  • Individual gas particles have mass but do not take up space
  • Gas particles only interact with one another and with the walls of the container when they collide
  • The higher the temperature the higher the kinetic energy
40
Q

Pressure and Boyles Law calculations

A

Pressure conversions:
Pressure given x Unit you want/unit you’re in
Ex, 750mmHg x 1atm/760mmHg

Boyle’s Law: P1V1=P2V2

41
Q

Kelvin Temperature scale and calculations with Charles and Gay-Lussacs Laws

A

Kelvin temperature scale: Designed so 0K is when a substance posses no kinetic energy. 0 degrees Celsius = 273K

42
Q

Combined gas law calculations

A

P1V1/T1=P2V2/T2

43
Q

Ideal gas law calculations

A

PV=nRT

*R=8.314

44
Q

Acid definition

A

A substance that ionizes water to produce one or more hydrogen ions

45
Q

Solution

A

A homogeneous (uniform) mixture of two or more substances

46
Q

Solvent

A

The base substance that has other substances dissolved in it

47
Q

Solute

A

The substance that is dissolving into the solvent

48
Q

Aqueous Solution

A

A solution that contains water (aq)

49
Q

Predicting the nature of a bond based on the electronegativity difference of bonding atoms.

A 
Completely Ionic Bond: 3.3EN
Mostly Ionic Bond: 1.7-3.3EN
Polar Covalent Bond: 0.5-1.7EN
Mostly Covalent Bond: 0-0.5EN
Completely Covalent Bond: 0EN
50
Q

S.T.P.

A

273K 101.3kPa

Grade 11 Exam Reviews (5 decks)

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