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61 Cards in this Set

  • Front
  • Back
Which one of the following is not an SI base unit?
a. mole
b. meter
c. gram
d. second
e. kelvin
c.
Select the answer that expresses the result of this calculation of the mean with the correct number of significant figures.

9.46g + 8.89g + 8.50g + 9.80g
--------------------------------------------
4

a. 9
b. 9.1
c. 9.13
d. 9.126
e. 9.1262
d.
You have a 4.58g sample of copper ore that contains 1.66g of oxygen. Malachite [Cu2CO3(OH)2] has a mass % of oxygen of 36.18%. Azurite [Cu2(CO3)2(OH)2] has a mass % of oxygen of 45.53%. Is the copper ore malachite or azurite?
a. malachite
b. azurite
a.
Which of the following statements about atoms and subatomic particles is/are false?
A Ernest Rutherford used the gold foil experiment to discover the existence of a dense, negatively charged nucleus
B Dalton thought that atoms were indivisible
C Robert Millikan performed the oil drop experiment
D J.J. Thompson discovered the existence of a negatively charged particle in atoms using a cathode ray tube.
E Dmitri Mendeleev is given credit for discovering the periodic table because he put the elements in order based on their atomic weight.
F Electrons and protons have equal and opposite charges
a. A, B and E
b. A and E
c. E and F
d. A
e. C and D
b.
Which of the following compounds is covalent?
a. ScI3
b. CaSO4
c. NH4Br
d. AlN
e. N2O5
e.
Which of the following elements exists as a diatomic molecule in its elemental form?
a. argon
b. titanium
c. hydrogen
d. boron
c.
The smallest unit into which a pure substance such as sugar or water can be divided, while still retaining its composition and chemical properties is a(n)_____.
a. ion
b. atom
c. particle
d. molecule
d.
TD or EX marking on glassware means...
a. the glassware was calibrated to dispense the measured amount of liquid by gravity, without additional force.
b. the glassware will deliver exactly the measured amount of liquid if blown out.
c. the glassware will deliver less than the required amount of liquid unless blown out.
d. the glassware was calibrated by the manufacturer to contain the amount of liquid when at the marked volume.
e. None of the above.
a.
Which of the following is NOT true:
a. Observation are natural phenomena and measured events
b. An experiment is a procedure to test a hypothesis
c. A hypothesis is a true statement
d. A theory is based on observations seen in experiments.
c.
Which of the following is a chemical change?
a. broiling a steak on a grill
b. boiling canned soup
c. carving a piece of wood
d. condensing water vapor into rainfall
a.
The area of a 15-inch pizza is 176.7 in2. Express this area in square centimeters.
a. 448.8 cm2
b. 27.39 cm2
c. 28,960 cm2
d. 69.57 cm2
e. 1140. cm2
e.
How many electrons are in the magnesium cation?
a. 24
b. 12
c. 14
d. 10
d.
Precision refers to how close your measurements are to:
a. the actual answer
b. one another
c. zero
d. your bench partner's answer
b.
Water vapor is less dense than ice because
a. molecules in the gas phase have more space between them than in solids
b. molecules in the gas phase are in constant motion
c. molecules in the gas phase have more kinetic energy than in solids
d. gaseous molecules have less mass
e. molecules in the gas phase have more potential energy than in solids
a.
Predict the physical state of tricontane (C30H62) at a temperature of 25 degrees Celcius. The melting point of tricontane is 66 degrees C and the boiling point is 450 degrees C.
a. gas
b. liquid
c. solid
c.
The empirical formula of a compound C12H14O6 is:
a. C6H7O3
b. C12H14O6
c. CH2O
d. C24H28O12
a.
The reaction of aluminum and sulfur produces aluminum sulfide. Write the formula of the product and indicate the type of bonding in this compound.
Al₂S₃
ionic
What two ions make up each of the following formulas? Be sure to include the charge for each.
CoSO₄
(H₃O)₃N
a) Co +2, SO₄ -2
b) H₃O +, N -3
Complete the following about the periodic table:
Name the element in group 10 and period 6.
Pt
What is the name of the group that contains Cs?
alkali metals
Name the element in group 4B and period 4.
Ti
Name the halogen in period 3.
Cl
Give an example of an inner transition element.
Nd
Name the metalloid in group 6A
Te
What is not a true statement about the following chemical reaction?
16Cu(s) + S8 (s) --> 8Cu2S (s)
a. For every 4 molecules of copper (I) sulfide produced, 8 atoms of copper are consumed
b. For every 2 moles of sulfur consumed, 16 moles of copper (I) sulfide are produced.
c. For every 16 grams of copper consumed, 1 gram of sulfur is required
d. For every 32 moles of copper consumed, 2 moles of sulfur are required
e. For every 16, moles of copper consumed, 8 moles of copper (I) sulfide are produced
c.
The smaller quantity of a substance in a solution is known as a(an):
a. molecule
b. solute
c. analyte
d. compound
e. solvent
b.
Identify the heterogeneous mixture.
a. blood
b. air
c. coffee
d. salt water
a.
The component in concrete that becomes hydrated is...
a. gravel
b. cement
c. sand
d. water
e. none of the above
b.
A compound contains 8 moles of water and 4 moles of CaSO₄. What is the formula of this hydrate?
a. 4 CaSO₄ * 8 H₂O
b. 2 CaSO₄ * H₂O
c. CaSO₄ * 2 H₂O
d. CaSO₄ * 8 H₂O
c.
What are the essential nutrients (elements) found in plant food?
I. sodium
II. nitrogen
III. potassium
IV. iron
V. phosphorus
VI. aluminum

a. I and IV
b. II only
c. IV and VI
d. II and III
e. II, II, V
e.
A (an) __________ absorbs water at room temperature
a. ionic
b. efflorescent
c. hydrate
d. hygroscopic
d.
Calculate the mass percent of sodium in sodium oxide.
a. 37.1%
b. 59.0%
c. 57.5%
d. 69.6%
e. 74.2%
e.
A compound has an empirical formula CH₂O. If its molecular mass is 150.13 g/mol, what is the correct molecular formula?
C₅H₁₀O₅
How many cesium ions are present in 0.276 mol Cs₂SO₄?
3.32 x 10^23 Cs ions
A solution is made by taking 54.62 g of K2CrO4 in enough water to make 250mL solution. What is the concentration of this solution?
a. 0.001125 M
b. 1.125 M
c. 0.0002813 M
d. 0.2813 M
e. 1.409 M
c.
b.
Write the correct name or formula for the following compounds

MoBr5 * 6H2O
Molybdenum (V) bromide hexahydrate
LiClO4
Lithium perchlorate
(NH4)2SO4
ammonium sulfate
Nitrous acid
HNO2
Aluminum acetate
Al(C2H3O2)3
Barium hydrogen carbonate
Ba (HCO3)2
What is the systematic name for the compound known as water?
dihydrogen monoxide
Select the gas with highest kinetic energy at 298K.
a. oxygen
b. carbon dioxide
c. water
d. hydrogen
e. All have the same kinetic energy
e.
Which of the following is a state function?
a. work
b. density
c. heat
d. enthalpy
d.
All of the following are assumptions (postulates) of the kinetic-molecular theory of gases EXCEPT
a. The gas molecules are in constant motion.
b. Collisions with the container wall cause pressure
c. The volumes of the molecules are small compared with the volume of the container
d. At a constant temperature, all molecules of the gas are moving at the same speed
e. The collisions between molecules are elastic
d.
Which of the following gases will be the slowest to diffuse through a room?
a. oxygen
b. neon
c. hydrogen
d. water
e. carbon dioxide
e.
What is the systematic name for the compound known as water?
dihydrogen monoxide
Select the gas with highest kinetic energy at 298K.
a. oxygen
b. carbon dioxide
c. water
d. hydrogen
e. All have the same kinetic energy
e.
Which of the following is a state function?
a. work
b. density
c. heat
d. enthalpy
d.
All of the following are assumptions (postulates) of the kinetic-molecular theory of gases EXCEPT
a. The gas molecules are in constant motion.
b. Collisions with the container wall cause pressure
c. The volumes of the molecules are small compared with the volume of the container
d. At a constant temperature, all molecules of the gas are moving at the same speed
e. The collisions between molecules are elastic
d.
Which of the following gases will be the slowest to diffuse through a room?
a. oxygen
b. neon
c. hydrogen
d. water
e. carbon dioxide
e.
What is the frequency of light with a 645nm wavelength?
4.65 x 10^14 s-1
In the Beer Lambert law A=E(w)bc, b is the
a. y-intercept
b. absorption
c. molar absorbivity
d. path (cell) length
e. solute concentration
d.
For a substance to be considered a strong electrolyte, it must
a. be an ionic compound
b. dissociate virtually completely into ions in solution
c. be highly soluble in water
d. contain both metal and nonmetal atoms
e. be a covalent compound
b.
What type of reactions can be utilized in a titration?
a. acid-base
b. redox
c. precipitation
d. all of the above
e. none of the above
d.
In a reaction, elemental silver loses an electron. Silver is said to be:
a. reduced
b. oxidized
c. an oxidizing agent
d. an anion
e. none of the above
b.
Which of the folloing is a diprotic acid?
a. H2Cr2O7
b. H3PO4
c. HC2H3O2
d. HClO4
a.
What is the oxidation number of sulfur in magnesium sulfite?
a. 0
b. 3
c. -2
d. 6
e. 4
e.
In the lab you performed an experiment that examines the relationship between the volume and pressure of a gas. Which variable(s) was held constant?
a. volume and pressure
b. temperature and number of moles of gas
c. pressure and temperature
d. number of moles of gas and pressure
b.
The following reactions:
Pb+2 (aq) + 2I- (aq) -->PbI2 (s)
2Ce+4 (aq) + 2I- (aq) -->I2(aq) + 2Ce+3 (aq)
NaOH(aq) + HNO2(aq) --> NaNO2 (aq) + H2O (l)
are examples of
a. precipitation, redox, and acid-base reactions, respectively
b. unbalanced reactions
c. precipitation, acid-base, and redox reactions, respectively
d. redox, acid-base, and precipitation reactions, respectively
e. acid-base reactions
a.
What is the concentration of potassium ions in 2 M potassium carbonate?
a. 2 M
b. 0.5 M
c. 4 M
d. 6 M
e. cannot tell
c.