Final Chemistry Exam

Tiny particles called atoms.

They form stable compounds

The concept of a mole.

A mole is simply a number

6.02x 10 to the power of 23.

Find the mass of something or find the number of atoms.

It is the ratio of mass in grams to the number of moles.

# of particles = n times (x) avagadros number

You can find the mass.

n=m/mm

Mol

Grams(g)

g/mol

Molarity

C=n/v

Mol

mol/L

Liters(L)

The law of conservation of mass.

The reactant

The product

The reacts= the products

A+B = AB

AB= A+B

A+BC =AC+B (the one that’s alone goes with the second element one the compound. The first goes by itself)

AB+CD=AD+CB ( the first element stays the same the second switches)

Very reactive and have one Valance electron.

2 valance electrons and some what reactive.

They are metals were multiple ions are possible

They make organic molecules and form covalent bond.

They are reactive and need one electron to form a stable Octet.

They have stable octets and are more dense as you go down the table.

They make bases in H2O and are bigger and more reactive as you move down the table.

They make bases in H2O difficult to “de-earth” and have high boiling and melting points

Shining high boiling and melting points.

Salts

They form single, double and triple bonds. They are brittle and do non conduct heat or electricity

They are Inert and non - reactive

They are shared but have a tendency to stay near the more electronegative atom.

It is called a slight negative or positive dipole.

N, O and F

Br2,I2,N2,Cl2,H2,O2 and F2

Have no fear of ice cold beer.

The chemical symbol surrounded by the number of valance electrons.

1. Write the chemical symbol for each element with the metal first. 2. Write the ionic charge above each symbol. 3. Crossover the ionic charges and write them below. Remove charges 4. Simply the numbers if necessary remove the 1’s.

1. Determine how many there are of the first non-metal. 2. Add the appropriate prefix before the non- metals name unless it is mono-. 3. Name the second non-metal with an appropriate prefix. 4. Change the ending of the last element to -ide.

1. Name the metal first 2. Name the non-metal and Change the ending to -ide. No prefixes.

1. Name the metal first. 2.determine the metals ionic charge. 3. Write the ionic charge using Roman numerals in brackets. 4. Name the non-metal changing the ending to -ide.

The same atomic number.

The amount of positively charged protons and negatively charged electrons.

Neutrons

They have the same mass.

Number of valance electrons and are in the same family.

The same number of electron shells and are in the same period.

You write the number of protons and neutrons in the centre and then put the number of electrons in a cloud like structure around.

This is a type of intra molecular force forms between a metal and a non - metal.

It is formed between two molecules of opposite charges. Electrons are stolen by the more electronegative atom.

It means it has a desire to get electrons.

F

A cation

An anion

Use Lewis diagrams and make sure nothing is alone.

Crystalline structures

Is a bond between two non- metals.

They share electrons to form stable electrons shells that satisfy the octet rule.

Covalent bonds

They are charged molecules containing covalent bonds.

They don’t conduct electricity.

A single is used when atoms share two electrons.

A double bond is used when atoms share four electrons.

A triple bond is used when atoms share six electrons.

1. Count up the total number of valance electrons you have to work with.2. Try forming all single bonds with all atoms involved first (include your lone pairs). Make sure you follow the octet rule with all atoms(remember exceptions)3. Count the number of electrons you used. If the number is the same as your count in step 1, you are done.if you have counted more electrons the number in step 1, you must begin forming multiple bonds.

Stoichiometry is using the proportional relationships in a chemical reaction to determine or calculate the amount of elements or compounds involved in a chemical change.

A mole ratio describes the ratio in which the substances combine.

They are used to predict, will happen if you had one substance changes

1. Balance the chemical equation(if needed)2. Set up a mole ratio or calculate the number of moles3. If you just calculated the number of moles set up a mole ratio.4. Find the answer for what the question is asking you.

Thermodynamics is the study of heat and temperature.

Energy is the capacity to do work.

Temperature is the measure of the agitation of the atoms and particles in a system.

Heat is the transfer of thermal energy when two systems with different temperatures come into contact with each other. Heat is a form of energy.

0th Law: Two things that come together at the same temperature with a third thing are all at the same temperature.1st Law: energy cannot be created or destroyed, only transferred from one state to another. This is the law of conservation of energy.2nd law: heat can only travel from a warmer object to a colder one. All systems tend to move from a state of higher order to less order. This, the total of entropy (the measure of randomness) of the universe will increase.3rd law: There is constant entropy at absolute zero. It is impossible to reach absolute zero.

System is a zone under observation.

Everything that is not contained with in the system is considered the surroundings/environment/universe.

Open, closed and isolated systems

In an open system, both energy and matter can move freely in and out of the system.

A campfire or beaker.

In a close system, energy can move in and out of the system, but matter cannot.

A tire or balloon

In an isolated system, neither energy or matter can be exchanged with the system.

A bomb calorimeter or a really good thermos.

It is due to the chemical nature of a substance. (Depends on there desire to get electrons)

Q= mc(delta T)

Joules (J)

Joules (J)

Grams (g)

J/g•c

(Tf-Ti) in degrees Celsius

The specific heat capacity of a substance is the amount of energy required to heat 1 g of a substance by 1°C.

Conduction

Convection (flow of air)

Radiation (microwave or sun)

Heat moves from two stationary objects in contact with each other.

Cooking with a frying pan

One of the object is of fluid. The faster the fluid moves. The more heat is transferred between objects.

Driving with your hand out the window or using the fan

Energy in the form of an electromagnetic wave propagates through the median until it contacts an object to the most common source of radiation is the sun.

Radiation can travel through a vacuum, such as interstellar space

The value of Q is negative, and the final temperature is less than the initial temperature

The value of Q is positive and the final temperature is more than the initial temperature

- m1cp1 (Tf -Ti) = m2cp2 (Tf -Ti)

M1 and m2 are in grams (g)

Cp1 and Cp2 are in J/ g•C

Tf and Ti are the change of temperature in degrees Celsius

Tf is the same for both sides or objects

The letter H

It is a word used to define the total amount of potential kinetic energy contained in a system at constant pressure

It is the measure of the vibrational translational and rotational movements of a substance.

Is the amount of energy that can be turned into kinetic energy.

It exists through the nuclear attraction between protons and electrons when they are together they are stable and in a low potential state however, if they if you move them apart, you’re just creating potential for them to combined and then doing so they give off a kinetic energy.

Delta H = Hproducts - Hreactants

Kilojoules (KJ)

Heat enters the system so it absorbs energy making it feel cold.

Positive

Heat leaves the system releasing energy and the system feels hot.

Negative

Solid to a liquid (melting)

Liquid to a gas

Gas to a liquid

Liquid to a solid

Fusion

Vaporization

Condensation

Solidification

Endothermic

Exothermic

Bond energy is the amount of energy required to break a specific chemical bond.

Endothermic

Exothermic

Delta Hr = delta Hbonds broken + delta Hbonds formed

KJ / mol

Positive

Negative

1. Draw a Lewis dot diagram for all species involved.2. Determine their bonds energies from table.3. Calculate the enthalpy change of the reaction4. Draw the energy balance diagram.

A thermodynamical equation is a balanced equation that includes the enthalpy of the reaction within the balance.

Intermolecular forces are between molecules

Intramolecular forces within molecules

1. Hydrogen bonds

2. Polar bonds

3. Van der Waals

1. Ionic

2. Covalent

3. Ionic and covalent

Hydrogen bonds are the strongest intermolecular bond. They occur when hydrogen is bonded with N, O, and F

Polar bonds occur between any other combinations and are not evenly spread out.

Van der Waals forces are any-other combination of forces that are evenly spread out. They are the weakest.

Random election displacement

Molar heat neutralization is the quantity of energy that is absorbed or released during the neutralization of one mole of an acid or a base.

1. Hydrocarbons with larger molecular weights have higher boiling points because of increased Van der Waals forces.2. Water is a liquid at room temperature because of H- bonds. CO2 is not.3. A geckos toes can stick to a wall because of extremely tiny hairs that create Van der Waals forces.4. Methanol is a liquid because it is polar, creating attractive forces between neighbouring molecules. CH4 is non- polar and is a gas at room temperature.

The solute is the less abundant quantity that dissolves in another.

The solvent is the liquid in greater quantity that contains the solute.

Water

They dissociate

The law of constant heat summation.

It applies for the delta H of dissociation and neutralization as well as any reaction whose heat of reaction is determined using a calorimeter.

If a reaction is broken down into several simple reactions, its enthalpy change is equal to the sum of the enthalpy changes of each of the simple reactions.

Kj/mol

Exothermic

Endothermic

Exothermic

Endothermic

Average reaction rate

Ideal reaction rate

Rreactants = - delta Quantity of R / delta t

Rproducts= delta Quantity of P/ delta t

Reaction rate of the reactants.

Reaction rate of the products

The quantity of reactants or products.

The final quantity minus the the initial quantity for the reactants and products respectively

The change in time (tfinal -tinitial)

That not all species are being consumed or produced.

The stoichiometric coefficients in the balanced chemical equation.

Reaction rate is simply the change in the quantity of a substance divided by the change in time over which it occurred.

(mol/L)/s

The coefficients of each species in the balanced chemical equation.

The reaction rates for each species involved in the reaction.

The coefficients of each species in the balanced equation.

Change in time (final time - initial time)

The change in concentration for each species

mol/L

Elastic and inelastic

The reactant particles hit each other and bounce off with no reaction.

Where the reactants hit each other with sufficient energy and orientation to cause a reaction

Reactant particles must have the correct orientation

Particles must have sufficient energy equal to or greater than the activation energy.

Activation energy is the minimum collision energy required for a reaction to occur.

It can be determined experimentally and form an energy/time graph.

-increase temperature (energy)

-increase concentration/ # of particles

-introduce a catalyst

-increase surface area

Many elementary reactions

Small reactions that take place

Pemto or Pico

A femto second is a billionth of a millionth of a second.

On a graph, this can be shown as a tangent.

A heterogeneous reaction

Homogenous

Intermolecular forces

The higher the bond energy the slower the reaction. Vise versa

The phase of the reactants

The bond energy

Greater force of attraction.

In a solid particles are very close and the forces are stronger then those between neighbouring molecules compared to liquids and gases.

The width of a hair

Intermolecular forces

1. Solid

2.Liquid

3. Gases

4. Aqueous ions

They typically have very high energy and are quite unstable.

The elementary reaction with the highest activation energy is considered the rate limiting step.

Graphically, table of values, and words

The average reaction rate of a chemical reaction is the change in the quantity of a reactant or product over a given length of time.

This can be shown as a secant between two points.

The instantaneous reaction rate of a chemical reaction is the reaction rate of a specific time during the reaction.

Aquarius ions react the fastest because they are composed of ionic charges which forces the molecules to be attracted or repulsed from each other.

The activation energy

Higher activation energies

The reaction rate of molecules with strong bond energies is typically very slow. Compounds containing triple and double bonds are slower than compounds containing single bonds

-kindling will burn faster then a large log

.- dust can catch fire faster than a large pile of dust.

- a small powder will dissolve faster than something that is solid.

The rate law is an expression relating the rate of a reaction to the concentration of the reactants.

Reaction rate

The rate constant

The stiochometric coefficients of the reactants in the balanced chemical equation of the elementary reaction.

mol/L•s

Fast reaction

Degree reaction

The degree of the reactants is the sum of the exponents for each reactant.

Only the concentration of gases and aqueous ions are considered in the rate law equation.

Solids and liquids are not considered in the rate law equation.

Catalyst are substances that increase the reaction rate without changing the result of the conversion and without being consumed by the reaction.

Homogeneous catalyst

Heterogeneous catalysts

The enthalpy of a reaction.

It lowers the activation energy (it takes less energy to react)

An inhibitor is a substance that reduces the reaction rate. It acts by increasing the activation energy of a chemical reaction.

The lock and key model is when something of a defined shape can only fit one type of molecule.

When a molecule will take the form of whatever it is required to be in.

A lock going in a door.

Pushing something into playdo.

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The ideal, simple and general gas laws

You have to first apply stoichiometric calculations involving mole ratios to identify the number of moles in either the products or reactants depending on what you are looking for.

Dalton's law of partial pressure states that the total pressure of a gas is the sum of the pressures of each individual species of gas.

Given the total pressure of the mixture, take the number of moles of this species divided by the total # of moles in a mixture.

The mole percentage

PV=nRT

Kpa

Litres (L)

mol

Kelvins (K)

To find all unknown variables given all of the others conditions are known

Ideal gases follow the kinetic molecular theory of gases and makes some ideal assumptions that arn't always true.

Real gases do not follow the kinetic molecular theory of gases while ideal gases do.

The general gas law is used to calculate the new conditions of a gas when one variable changes.

That for a given quantity of ideal gas held at constant volume the pressure is always proportional to the absolute temperature.

P1/T1 = P2/T2

At the same temperature and pressure the volume of the gas is directly proportional to the number of moles

V1/n1 = V2/n2

At constant temperature for a given quantity of ideal gas the pressure is always inversely proportional to the volume.

P1V1 = P2V2

At a constant pressure for a given quantity of ideal gas, the volume is always proportional to the absolute temperature.

V1/T1 = V2/T2

P = F / A

Newtons (N)

Meters squared

Pascals (Kpa), Atmospheres (atm), Millimeters of mercury (mmHg)

760 mmHg = 101.325Kpa = 1 atm

Is an instrument used to measure air pressure.

mmHg

The pressure is measured as the height of the column.

There is no height different so the pressure is equal.

h2 - h1

1. h2 - h1

2. P= Ph + Patm

Diffusion is the tendency of gas molecules to disperse in all directions until they are uniformly distributed.

Diffusion is caused by the 2nd postulate of the kinetic molecular theory of gases which states that all particles are constantly in motion in straight lines in all directions.

The Scent of perfume travelling through a room

Effusion is a much slower process in which a gas travels across a membrane with microscopic pores.

The shrinking of a balloon with time as air elapses.

Gortex is used for rain jackets because it has small pores which allows water from sweat in the form of gas to effuse away from the body.

Water droplets are much larger then the pores of the jacket so they cannot pernitrate through to the skin and the wearer stays dry.

The molecular weights of those gases

Grahams law states that the velocities between two gases is inversely proportional to the square root of their molar masses.

It is a hypothetical model based on experimental observations used to explain the theory of an ideal gas

Solid, Liquid, gas, Plasma, Bose - Einstein Condensate

Plasma is the fourth state of matter and consists of ionized particles

Fire

Plasma

1. All particles are infinitely small and the size of a particle is negligible compared to the container that it holds (Gases don't take up space)

2. The particles of gas are in constant motion and move in straight lines.

3. The particles of gas do not exert any force of attraction or repulsion on each other. No energy is lost during a collision

4.The mean kinetic energy of the particles is directly proportional to thier absolute temperature. (Hot particles move faster then cold particles.)

Vibrational

Rotational

Translational

Only Vibrational

Vibrational and Translational

Vibrational

Translational

Rotational

Liquids and solids

There are compressible and will expand to adopt the volume of their container.

They have a fixed mass but will take the shape of their container.

If the temperature increases because the velocity of the particles will also increase

In increase in temperature will allow particles to overcome the attractive force of neighboring molecules to turn into a liquid.

The intermolecular bonds exhibited by the molecules in a liquid can be overcome and the particles will evaporate into the gas phase taking the energy with them.

Ek = 1/2mv(squared)

Joules(J)

Kilograms (kg)

Meters per second (m/s)

The lower the velocity. vise versa

Nitrogen at 78% , Oxygen at 21%, Argon less then 1%, and Carbon Dioxide at 0.03%

Neon, Helium, Methane, Krypton, Xenon, Hydrogen, Ozone and radon,

It contains triple bonds which require a lot of energy to break.

In the roots of plants

In marshlands and landfills resulting from anaerobic (no oxygen) fermentation of organic matter.

Sequestered in the ocean floor, the permafrost in the nornthern climates and in ruminant animals such as cows.

A green house gas

Forest fires

CO2, H2O, CO, SO4

Poisonous H2S

A spectacular light display where ionized particles from the sun pernitrate the atmosphere close to the magnetic poles creating light.

- Preserves food

- Inflates tires

- Makes NH3 used in fertilizers

- Scuba gear

- Causes fires

- Medicine

- Neon Lights

- Weather balloons

- In Windows

- Paintball

- Tools/ Nail gun

- Hydraulics

- Fire extinguishers

- Pop cans

- Food preservatives

Have an asphyxiating (Can't breath) or suffocating effect

A toxic gas that can be monitored in your home.

Radon is also dangerous in your home and can accumulate in the basement through cracks in the floor.

Oxygen

Methane, Ethane, Propane, Butane.

A clean fuel because it does not release CO2 into the atmosphere.

In 1937 the great Hindenburg disaster occurred when a blimp containing hydrogen caught on fire.

Helium

Ozone

O3

In the stratospheres ozone protects us from UV rays by absorbing their energy.

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