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1) Which of the following is NOT a laboratory safety rule?
a) You should never mix acids with bases
b) You should tie back your long hair
c) You should never add water to acid
d) All of the above are valid safety rules
2) What piece of laboratory equipment is best-suited foraccuratelymeasuring the volume of
a liquid?
a) graduated cylinder
b) beaker
c) Erlenmeyer flask
d) more than one of the above
3) Which piece of laboratory equipment can be used to store chemicals for long periods of
time?
a) buret
b) evaporating dish
c) beaker
d) more than one of the above
4) The independent variable in an experiment is:
a) The variable you hope to observe in an experiment.
b) The variable you change in an experiment .
c) The variable that isn’t changed in an experiment.
d) none of these is correct
5) “Qualitative results” refer to:
a) Results that can be observed during an experiment.
b) Results that are difficult to observe during an experiment.
c) Results thatrequire numerical data.
d) none of these is correct.
6) When drawing a graph that measures family average income over a period of 50 years,
the independent variable is:
a) Income
b) Average
c) Years
d) It is impossible to say
7) Accuracy is definedas:
a) A measure of how often an experimental value can be repeated.
b) The closeness of a measured value to the real value.
c) The number of significant figures used in a measurement.
d) None of these
8) How many significant figures are present inthe number 10,450?
a) three
b) four
c) five
d) none of these
9) What is the appropriate SI unit for distance?
a) centimeters
b) inches
c) meters
d) kilometers
10) How many decimeters are there in 15 centimeters?
a) 150 dm
b) 1.5 dm
c) 0.15 dm
d) none of these
11) How many kilograms are there in 4.21 pounds? There are 2.2 pounds in 1 kilogram.
a) 9.26 kg
b) 1.91 kg
c) 0.523 kg
d) none of these
12) A homogenous material is defined as being:
a) An element
b) Any material with uniform composition
c) Synonymous with “solution”
d) More than one of these
13) An example of a chemical property is:
a) density
b) mass
c) acidity
d) solubility
14) “Exothermic” processes:
a) Absorb energy
b) Give off energy
c) Have no energy change
d) It is impossible to predict the energy change of an exothermic process.
15) Intrinsic properties are properties that:
a) Don’t depend on the amount of material present.
b) Depend on the amount of material present.
c) Cannot be measured without performi ng a chemical reaction.
d) None of the above is correct.
16) What is the density of an object with a volume of 15 mL and a mass of 42 grams?
a) 0.352 g/mL
b) 2.80 g/mL
c) 630 g/mL
d) None of the above is correct.
17) Which of the following is not one of Dalton’s laws?
a) Atoms are indestructible.
b) Atoms of the same element have isotopes with different masses.
c) Atoms of different elements have different chemical and physical properties.
d) All of these are examples of Dalton’s laws.
18) The “plum pudding” model of the atom was devised by:
a) Dalton
b) Democritus
c) Rutherford
d) none of the above answers is correct
19) Bohr’s model of the atom was able to accurately explain:
a) Why spectral lines appear when atoms are heated.
b) The energies of the spectral lines for each element.
c) Why electrons travel in circular orbits around the nucleus.
d) none of the above answers is correct.
20) What subatomic particle has a mass of one atomic mass unit?
a) proton
b) neutron
c) electron
d) more than one of the above
21) How many electrons does iron have?
a) 26
b) 30
c) 56
d) It depends on the isotope of iron
22) True or false: All isotopes are radioactive.
a) True
b) False
23) Mass spectrometers separate isotopes of different elements based on their:
a) mass
b) electric charge
c) mass divided by electric charge
d) none of these
24) What percent of atoms of magnesium have a mass of exactly 24 amu?
a) 100%
b) 70%
c) 30%
d) 0%
25) The colors of light given off when a sampl e is heated corresponds to:
a) The energy difference between the ground state and excited state of an element.
b) The amount of energy added to the sample.
c) The heat of the element.
d) None of the above
26) “Line spectra” are caused primarily by:
a) The existence of many ground states in an atom
b) The existence of many excited states in an atom
c) The existence of many atoms in a typical sample
d) None of the above
27) A continuous spectrum is caused primarily by:
a) The presence of so many ex cited states that the lines all blur together into a
rainbow.
b) The presence of so many ground states that the lines all blur together into a
rainbow.
c) The presence of many atoms in a typical sample.
d) None of the above
28) Which of the following is true of the distance of an electron from the nucleus of a
1
H
atom?
a) It is 1 amu.
b) It remains constant over time.
c) itsdistance at any given time can only be predicted by looking at a
“wavefunction”.
d) It is impossible to say where an electron will be at any given time.
29) Orbitals hold:
a) A maximum of one electron each
b) A maximum of two electrons each
c) A number of electrons that depends on the energy level.
d) A number of electrons that depends on the type of orbital.
30) Which type of orbital looks like a figure -8 when drawn?
a) s-orbital
b) p-orbital
c) d-orbital
d) f - orbital
31) Which of the following is not an allowed value for the angular momentum quantum
number of an atom?
a) -1
b) 0
c) +1
d) more than one of the above is disallowed
32) The magnetic quantum number of an orbital defines:
a) The energy level of the orbital
b) The shape of the orbital
c) The spatial orientation of the orbital
d) The spin of the electrons in the orbital
33) Which of the following typically has a low melting point?
a) metals
b) nonmetals
c) metalloids
d) transition metals
34) The difference between a “family” and a “group” in the periodic table is that:
a) Families are columns and groups are rows.
b) Families are rows and groups are columns.
c) Families determine the energy level of an element and groups determine their
properties.
d) None of the above is true.
35) Which of the following elements has three valence electrons?
a) lithium
b) boron
c) nitrogen
d) more than oneof the above
d) none of these answers is correct.
37) What section of the periodic table is a very strong oxidizer?
a) alkali metals
b) lanthan ides
c) halogens
d) none of these answers is correct.
38) Which element has the largest atomic radius?
a) fluorine
b) carbon
c) tin
d) iodine
39) The shielding effect explains why:
a) the electronegativity of fluorine is greater than that of bromine
b) the electronegativity of fluorine is greater than that of boron
c) the electronegativity of fluorine is smaller than that of gallium
d) none of these answers is correct
40) The octet rule explains why:
a) the electronegativity of fluorine is gre ater than that of bromine
b) the electronegativity of fluorine is greater than that of boron
c) the electronegativity of fluorine is smaller than that of gallium
d) none of these answers is correct
41) Cations have:
a) Positive charge
b) Negative charge
c) No charge
d) It is impossible to predict the charge on a cation.
42) Which pair of atoms would most likely form an ionic compound when bonded to each
other?
a) calcium and fluorine
b) silicon and nitrogen
c) two oxygen atoms
d) none of the ab ove would probably form an ionic compound
43) Which of the following is NOT a property of a salt?
a) They have ordered packing arrangements called “lattices”
b) They conduct electricity when dissolved in water or molten.
c) They have a low melting point but a high boiling point.
d) They are brittle.
44) The chemical name for Fe
2O3is:
a) iron oxide
b) iron (II) oxide
c) iron (III) oxide
d) iron (VI) oxide
45) The percent composition of aluminum in aluminum (III) hydroxide is:
a) 50%
b) 25%
c) 14%
d) none of these answers is correct.
46) Hydrates are defined as:
a) compounds with water molecules attached to them.
b) compounds that have had their water molecules removed
c) compounds that have been heated to high temperatures
d) none of thes e answers is correct.
47) Why do two nonmetals generally form covalent bonds with one another?
a) They have similar sizes
b) They have similar electronegativities
c) Nonmetals prefer to share electrons rather than transfer them
d) None of the above
48) Why do covalent compounds usually have lower melting and boiling points than ionic
compounds?
a) No bonds need to be broken to melt a covalent compound.
b) The intermolecular forces in ionic compounds are weaker than those in covalent
compounds.
c) Covalent molecules have higher electron affinities than ionic molecules.
d) None of the above is correct.
49) Why doesn’t water conduct electricity well?
a) Huh? Water is an excellent conductor of electricity!
b) Pure water contains very few ions.
c) The hydrogen bonding in water cause the molecules to move slowly from one
place to another.
d) None of the above is correct.
50) N2S3is properly named:
a) nitrogen sulfide
b) nitrogen (III) sulfide
c) nitrogen (II) sulfide
d) none of these
51) The difference between a molecular and structural formula is that:
a) Molecular formulas give you the ratios of the elements in a compound, while
structural formulas tell you how many atoms of each element are present.
b) Molecular formulas tell you where th e atoms in a compound are, while structural
formulas don’t.
c) Molecular formulas don’t tell you where the atoms in a compound are, while
structural formulas do.
d) None of the above is correct.
