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60 Terms
1
chlorine
halogen used in the disinfection of drinking water and the synthesis of medicines, crop-protection chemicals, and PVC plastics
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2
hydrogen
the most abundant element in the universe
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3
helium
noble gas used as a lifting gas in airships and weather balloons, as an extremely low-temperature coolant, and as a laser medium
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4
hydrogen
isotopes are commonly called protium, deuterium, and tritium
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5
nitrogen
extracted from the air and used to make artificial fertilizers and explosives
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6
oxygen
a gas found in air that is necessary for the survival of human and animals
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7
oxygen
ozone is an allotrope of this element
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8
fluorine
halogen used in dental hygiene and in the manufacture of refrigerants
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9
phosphorus
exists in an unstable white allotrope and a more stable red allotrope; used to make matches and some fertilizers
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10
sulfur
extracted from petroleum and natural used to make an important gas by the Claus process; industrial acid
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11
metallurgy
the science of extracting metals from their ores and preparing them for use
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12
electrolytes
substances that dissolve in water to produce ions that can conduct an electrical current
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13
Le Chatelier's
the effects of changes on equilibrium systems is described by _________ principle
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14
kinetics
the study of reaction rates and pathways is chemical _____?
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15
activation energy
the minimum kinetic energy that a molecule must possess to undergo a chemical reaction is the _________?
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16
catalyst
a substance that increases the rate of a chemical reaction without being consumed in the reaction is a _________?
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17
sodium
alkali metal found in lye, washing soda, baking soda, and table salt
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18
aluminum
the most abundant metal in the earth's crust; a lightweight metal widely used to make aircraft, spacecraft, and beverage cans
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19
iron
the second most abundant metal in the earth's crust; a lightweight metal widely used to make aircraft, spacecraft, and beverage cans
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20
gold
the most malleable and ductile metal known
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21
platinum
precious metal used in automotive and industrial catalysts
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22
silicon
most common semimetal; found in computer chips, glass, and sand
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23
iron
the metal most commonly refined by means of blast furnaces
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24
calcium
alkaline earth metal that helps compose limestone, slaked lime, and cement
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25
copper
metal used in electrical wiring and as a component of brass and bronze
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26
Which of the following changes would not increase the rate of a chemical reaction?
diluting reactant concentrations
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27
A solution that contains as much dissolved solute as possible under equilibrium conditions is said to be ______?
saturated
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28
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
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29
Which of the following statements about catalysts is true?
a catalyst increase the reaction by lowering the reaction's activation energy
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30
The rate of a chemical reaction is usually measured as ______?
the change in concentration of a given substance per unit of time
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31
In a solution of sodium chloride in water, water is the ______?
solvent
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32
Which of the following statements best describes a system at equilibrium?
Rates of forward and reverse reactions are equal
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33
The flow of solvent through a semipermeable membrane from a more dilute solution to a more concentrated solution is called
osmosis
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34
A mixture of two or more metals, usually melted together, is a ________?
alloy
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35
A mixture containing tiny clumps or particles that remain suspended within the mixture and will not settle out is ______?
colloid
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36
If the temperature of a chemical reaction is increased from 20C to 30C, we would ordinarily expect the reaction rate to __________?
double
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37
T/F: a nonpolar substance will be more likely to dissolve in a polar solvent than in a nonpolar solvent
F, polar
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38
T/F: a factor that causes a change in an equilibrium system is called a disturbance
F, stress
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39
T/F: protein catalysts found in living things are enzymes
T
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40
T/F: The energy diagram below represents an endothermic reaction
T
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41
T/F: if a nonvolatile solute such as glucose is added to water, the boiling point will increase
T
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42
T/F: When a gas is dissolved in water, decreasing the temperature tends to decrease the solubility of the gas
F, increase
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43
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
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44
Removing the hydrogen iodide as soon it is formed would shift the equilibrium to the ________?
right
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45
Increasing the pressure would shift the equilibrium to the _______?
No shift would occur
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46
Adding a catalyst to the system would cause the concentration of HII to ________?
remain unchanged
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47
Increasing the temperature would shift the equilibrium to the ________?
left
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48
Adding hydrogen to the system would cause the concentration of HI to shift to the ________?
right
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49
Adding iodine vapor to the system would shift the equilibrium to the _______?
right
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50
Removing hydrogen iodide from the system would cause the concentration of iodine to __________?
decrease
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51
What is the molarity of a solution containing 6.0 mol NaCL dissolved in 12 L of water?
0.50 M
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52
For the reaction 3 Fe9 (s) + 4 H2 (g) in what direction does adding a catalyst shift the equilibrium
No shift would occur
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53
For the reaction AgH2C2O3 -> Ag (aq) + H2C3O2 (aq), in what direction does an increase in pressure shift the equilibrium
No shift would occur
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54
Write the equilibrium constant expression for the reaction 2 NO(g) + Br2 -> 2 NOBr (g)
K = NOBr2
No2Br2
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55
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
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56
Write the equilibrium constant expression for the reaction CaCl2(s) + 2 HCl(aq) -> CaCl2(aq)
K = CaCl2CO2
HCl2
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57
Write the solubility product constant expression for aluminum hydroxide
K = AL-3OH-3
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58
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
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59
Calculate K
290
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60
Calculate NO
1.1 x 10 -5 M
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