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chlorine
halogen used in the disinfection of drinking water and the synthesis of medicines, crop-protection chemicals, and PVC plastics
hydrogen
the most abundant element in the universe
helium
noble gas used as a lifting gas in airships and weather balloons, as an extremely low-temperature coolant, and as a laser medium
hydrogen
isotopes are commonly called protium, deuterium, and tritium
nitrogen
extracted from the air and used to make artificial fertilizers and explosives
oxygen
a gas found in air that is necessary for the survival of human and animals
oxygen
ozone is an allotrope of this element
fluorine
halogen used in dental hygiene and in the manufacture of refrigerants
phosphorus
exists in an unstable white allotrope and a more stable red allotrope; used to make matches and some fertilizers
sulfur
extracted from petroleum and natural used to make an important gas by the Claus process; industrial acid
metallurgy
the science of extracting metals from their ores and preparing them for use
electrolytes
substances that dissolve in water to produce ions that can conduct an electrical current
Le Chatelier's
the effects of changes on equilibrium systems is described by _________ principle
kinetics
the study of reaction rates and pathways is chemical _____?
activation energy
the minimum kinetic energy that a molecule must possess to undergo a chemical reaction is the _________?
catalyst
a substance that increases the rate of a chemical reaction without being consumed in the reaction is a _________?
sodium
alkali metal found in lye, washing soda, baking soda, and table salt
aluminum
the most abundant metal in the earth's crust; a lightweight metal widely used to make aircraft, spacecraft, and beverage cans
iron
the second most abundant metal in the earth's crust; a lightweight metal widely used to make aircraft, spacecraft, and beverage cans
gold
the most malleable and ductile metal known
platinum
precious metal used in automotive and industrial catalysts
silicon
most common semimetal; found in computer chips, glass, and sand
iron
the metal most commonly refined by means of blast furnaces
calcium
alkaline earth metal that helps compose limestone, slaked lime, and cement
copper
metal used in electrical wiring and as a component of brass and bronze
Which of the following changes would not increase the rate of a chemical reaction?
diluting reactant concentrations
A solution that contains as much dissolved solute as possible under equilibrium conditions is said to be ______?
saturated
The theory that when two molecules collide and chemically react they form a short-lived activated complex before breaking apart to form the products is the _______?
transition-state
Which of the following statements about catalysts is true?
a catalyst increase the reaction by lowering the reaction's activation energy
The rate of a chemical reaction is usually measured as ______?
the change in concentration of a given substance per unit of time
In a solution of sodium chloride in water, water is the ______?
solvent
Which of the following statements best describes a system at equilibrium?
Rates of forward and reverse reactions are equal
The flow of solvent through a semipermeable membrane from a more dilute solution to a more concentrated solution is called
osmosis
A mixture of two or more metals, usually melted together, is a ________?
alloy
A mixture containing tiny clumps or particles that remain suspended within the mixture and will not settle out is ______?
colloid
If the temperature of a chemical reaction is increased from 20C to 30C, we would ordinarily expect the reaction rate to __________?
double
T/F: a nonpolar substance will be more likely to dissolve in a polar solvent than in a nonpolar solvent
F, polar
T/F: a factor that causes a change in an equilibrium system is called a disturbance
F, stress
T/F: protein catalysts found in living things are enzymes
T
T/F: The energy diagram below represents an endothermic reaction
T
T/F: if a nonvolatile solute such as glucose is added to water, the boiling point will increase
T
T/F: When a gas is dissolved in water, decreasing the temperature tends to decrease the solubility of the gas
F, increase
T/F: A chemical system in which the rates of reaction in opposite directions have equalized so that the concentration of reactants and products is constant is in a state of chemical equilibrium
T
Removing the hydrogen iodide as soon it is formed would shift the equilibrium to the ________?
right
Increasing the pressure would shift the equilibrium to the _______?
No shift would occur
Adding a catalyst to the system would cause the concentration of HII to ________?
remain unchanged
Increasing the temperature would shift the equilibrium to the ________?
left
Adding hydrogen to the system would cause the concentration of HI to shift to the ________?
right
Adding iodine vapor to the system would shift the equilibrium to the _______?
right
Removing hydrogen iodide from the system would cause the concentration of iodine to __________?
decrease
What is the molarity of a solution containing 6.0 mol NaCL dissolved in 12 L of water?
0.50 M
For the reaction 3 Fe9 (s) + 4 H2 (g) in what direction does adding a catalyst shift the equilibrium
No shift would occur
For the reaction AgH2C2O3 -> Ag (aq) + H2C3O2 (aq), in what direction does an increase in pressure shift the equilibrium
No shift would occur
Write the equilibrium constant expression for the reaction 2 NO(g) + Br2 -> 2 NOBr (g)
K = NOBr2
No2Br2
Which of the following would not cause the reaction 2Al(s) + 6 HCl(aq) -> 3 H2 (g) + 2 AlCl3 (aq) to shift to the right?
increasing the pressure o the reaction chamber
Write the equilibrium constant expression for the reaction CaCl2(s) + 2 HCl(aq) -> CaCl2(aq)
K = CaCl2CO2
HCl2
Write the solubility product constant expression for aluminum hydroxide
K = AL-3OH-3
supersaturated
The solubility product of Ag2Co3 is 8.1 x 10-12. Is a 1.5 x 10-4 M solution of Ag2NO3, saturated, unsaturated, or supersaturated
Calculate K
290
Calculate NO
1.1 x 10 -5 M
Note 
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