Chemistry

Front 1

What are monatomic and polyatomic ions?

Back 1

monatomic ions are single atoms that gain/lose electrons. Polyatomic ions are a group covalently charged atoms

Front 2

where are the transition metals found on the periodic table?

Back 2

the D block

Front 3

What elements exsist as diatomic molecules?

Back 3

fluorine (F2), chlorine (Cl2), bromine (Br2), iodine (I2),astatine (At2),hydrogen (H2), nitrogen (N2), oxygen (O2)

Front 4

what is the limiting reactant?

Back 4

is the chemical that determines how far the reaction will go before the chemical in question gets used up, causing the reaction to stop.

Front 5

What is the excess reactant?

Back 5

The reactant in a chemical reaction that remains when a reaction stops when the limiting reactant is completely consumed. The excess reactant remains because there is nothing with which it can react.

Front 6

What is the difference between the theoretical yield and the actual yield?

Back 6

Amounts of products calculated from the complete reaction of the limiting reactant is called theoretical yields, whereas the amount actually produced of a product is the actual yield

Front 7

State Avogadros Law.

Back 7

Avogadro's Law states that under conditions of constant pressure and temperature, there is a direct relationship between the volume and number of moles for an ideal gas.

Front 8

What is STP?

Back 8

the standard molar volume of a gas. 22.4 L

Front 9

What is Graham's Law of Effusion?

Back 9

it states that the rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of thier molar masses.

Front 10

Use the Kinetic Molecular Theory to explain the properties of solids: density, compressibility, ability to diffuse, fluidity, definite volume and definite shape.

Back 10

Density: Solids are very dense because the particles of a solid are more closely packed together. Solids are considered incompressible. Diffusion does occur but extremly slow. They have definite volume beause their particals are packed closely together. They have definite shape without a container.

Front 11

Use the Kinetic Molecular Theory to explain the properties of liquids: density, compressibility, ability to diffuse, fluidity, definite volume and definite shape.

Back 11

At the same temp and pressure different liquids can differ greatly in density. Liquids are much less compressible then gases because liquid particals are more closely packed together. Any Liquid gradually diffuses throughout any other liquid in which it can dissolve, as temperature increases diffusion occurs more rapidly. Molecules will flow or glide over one another, but stay toward the bottom of the container. Motion is a bit more random than that of a solid. A liquid can be described as a form of matther that has definite volue and takes the shape of its container.

Front 12

Use the Kinetic Molecular Theory to explain the properties of gases: density, compressibility, ability to diffuse, fluidity, definite volume and definite shape.

Back 12

Molecules are in continual straightline motion. The kinetic energy of the molecule is greater than the attractive force between them, thus they are much farther apart and move freely of each other.

Front 13

What is the difference between amorphous and crystalline solids?

Back 13

Crystalline solids are arranged in fixed geometric patterns or lattices. Amorphous solids are solids with random unoriented molecules.

Front 14

Name and give exaples of 5 changes of state.

Back 14

solid->Liquid(melting ice->water

Solid->Gas (sublimation)
Dry ice->CO2 gas

Liquid->solid(freezing)
water->ice

Gas->Liquid(condensation)
water vapor->water

Gas->Solid(decomposition)
water vapor->ice

Front 15

What is endothermic and exothermic?

Back 15

endothermic properties it must absorb heat from its surroundings. If heat is produced when the melting action takes place it is exothermic.

Front 16

What is a suspension?

Back 16

a mixture in which fine particles are suspended in a fluid where they are supported by buoyancy. Suspensions separate on standing. The mixture of particles can be separated by filtration.

Front 17

what is a colloid?

Back 17

A homogeneous mixture with solute particles larger than a solution, but smaller than a suspension. Fog and milk are examples of colloids.

Front 18

what is a solution?

Back 18

A solution is a homogeneous mixture of one or more solutes dissolved in a solvent.Solutions are transparent. You can see through them.

Front 19

what makes water a polar molecule?

Back 19

Electronegative atoms are bullies. They hog electrons. In water, Oxygen pulls the electrons away from Hydrogen as much as it can. A polar molecule means that there is a greater charge on one side of the molecule than the other. In this case, there is a greater negative charge on the Oxygen.

Front 20

What is a saturated solution?

Back 20

A solution that contains the maximum amount of dissoleved solute.

Front 21

what is a unsaturated solution?

Back 21

a solution that cotains less solute than a saturated solution under the existing conditions.

Front 22

what is a supersaturated solution?

Back 22

a solution that contains more dissolved solute than a saturated solution contains under the same conditions.

Front 23

explain the effect of temperature on the solubility of gases and solids in liquid solvents.

Back 23

As the temperature increases, the solubility of a gas decreases.When a solid dissolves in a liquid, a change in the physical state of the solid analogous to melting takes place. Heat is required to break the bonds holding the molecules in the solid together.

Front 24

what is the difference between a strong electrolyte and and weak electrolyte?

Back 24

A Weak Electrolyte does not completely dissociate. Weak Bases and Weak Acids are generally weak electrolytes. Strong Electrolyte completely dissociates. Stong acids and bases are good examples.

Front 25

What are 5 general properties of acids?

Back 25

1. Aqueous solutions of acids have a sour taste.
2.Acids change the color of acid-base indicators
3.Some acids react with active metals to release hydrogen gas.
4. Acids react with bases to produce salts and water.
5.Acids conduct electric current.

Front 26

What are 5 general properties of bases?

Back 26

1.Aqueous solutions of bases taste bitter.
2.Bases change color of acid-base indicators.
3.Dilute aqueous solutions of bases feel slippery.
4.Bases react with acids to produce salts and water.
5.Bases conduct electic current.

Front 27

What is the Bronsted-Lowry definition of acids and bases?

Back 27

A Bronsted-Lowry (BL) acid is defined as any substance that can donate a hydrogen ion (proton) and a Bronsted-Lowry base is any substance that can accept a hydrogen ion (proton).

Front 28

What is the Arrhenius definition of acids and bases?

Back 28

Arrhenius suggested that acids are compounds that contain hydrogen and can dissolve in water to release hydrogen ions into solution.Arrhenius defined bases as substances that dissolve in water to release hydroxide ions (OH-) into solution.

Front 29

what are the products of neutralization reactions?

Back 29

The neutralization reaction of an acid with a base will always produce water and a salt.

Front 30

What is pH a measurement of? pOH?

Back 30

The pH is a measure of how acidic or basic (or alkaline) a liquid or solution is. pOH is a measure of the hydroxide ion concentration.

Front 31

what can be determined by doing titration?

Back 31

The chemically equivalent volumes of acidic and basic solutions.

Front 32

How can you tell when you have reached the end point during titration?

Back 32

the indicator changes color.

Front 33

what is the equivalence point?

Back 33

the point at which two solutions used in titration are present in chemically equivalent amounts.