Prepare for your Chemistry final exam with these practice questions and answers. This covers atomic structure, chemical bonding, reactions, and stoichiometry calculations.
Q: 1-Chemistry is the study of
Answer: matter
Q: 2-Which physical state is characterized by a indefinite shape and definite volume
Answer: Liquid
Q: 3-Whether a substance is a solid, liquid, or gas depends on its
Answer: Temperature
Q: 4-Tea, water, and sugar evenly distributed in the glass is an example of a(an)
Answer: Mixture
Q: 5-In a homogenous mixture there is (are)____________ phase(s)
Answer: One
Q: An atom is the smallest unit that has the properties of a particular ____________
Answer: Element
Q: The difference between a compound and a mixture is that a compound has a ______________ chemical composition whereas a mixture has a ___________ chemical composition.
Answer: definite; variable
Q: The two-letter designation for the element cobalt is
Answer: Co
Q: CH4 is a ____________ molecule and a __________ molecule.
Answer: Pentatomic; heteroatomic
Q: 10-XeF4 is a(n) _________________.
Answer: compound
Q: If you have a deciliter then you have ___________ Liters.
Answer: 14
Q: The formula Fe2(CO3)3 represents ______________ atoms
Answer: 0.1 Liters
Q: There are _________ centimeters in one kilometer
Answer: 100,000
Q: The number 1.02340 has ________ significant figures.
Answer: 6
Q: 15- 0.00000100 has ________ significant figure(s),
Answer: 3
Q: The number 2.81298 will become __________ when you round to 4 significant figures
Answer: 2.813
Q: The multiplication of 9.0021 times 4.430 will have _______ significant figures.
Answer: 4
Q: Today you are at the lake playing on a rope swing. Your friend from Europe tells you about a rope swing at his home town. He says it is 307.848 cm above the lake. He says his swing is higher than the one you are at here in the Okanogan Valley. Being scientific and diplomatic you show him that 307.848 cm is ___________ than your 18.4 ft above the water rope swing.Conversion: 1 inch = 2.54 cm; 1 foot = 12 inches
Answer: Lower
Q: The density of pure water is 1.00 g/ml. You add a liquid to a container of water. This liquid weighs 12.1 grams and has a volume of 20 ml. Based on your calculation the liquid is ____________ dense than the water as as such it will __________ when added to a container of water
Answer: less; float
Q: 20- At 373 Kelvin water will change from a liquid to a gas. What temperature is this expressed in Fahrenheit?
Answer: 212 degrees
Q: The mass of an electron is _____________ to that of the neutron.
Answer: significantly less
Q: An element with an atomic number of 12 is___________ and it will have ____________ protons and ________________ electrons
Answer: Magnesium; 12; 12
Q: The mass number of an element is 204 and the atomic number is 81. From this information I know that there are __________ protons, _____________ neutrons, and ____________ electrons.
Answer: 81; 123; and 81
Q: I have two atoms. One has a mass number of 23 and the other has a mass number of 24. Both have atomic numbers of 11. From this I can say that these two atoms are _____________
Answer: Isotopes of sodium
Q: 25- The octet rule is based on the observation that atoms with gain, loses, or share electrons in order to get _____________ electrons in their valence shell.
Answer: 8
Q: Elements in Group IA are referred to as _____________ and in a chemical reaction will ______________ (an) electron(s) giving it a ____________ charge.
Answer: Alkali Metals; lose; positive
Q: How many Electron Shells are theoretically possible
Answer: 7
Q: How many orbitals does a p-subshell potentially have?
Answer: 3
Q: How many electrons are found in the 2nd energy shell of an Aluminum atom
Answer: 8
Q: 30- What is the valence shell for the element Nitrogen
Answer: 2
Q: How many electrons can a d subshell hold?
Answer: 10
Q: What is the electron configuration for calcium
Answer: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2
Q: What is the valence shell electron configuration for potassium?
Answer: 4s1
Q: Group IA through Group VIIA are called the
Answer: Representative elements
Q: 35- 1s22s22p63s23p6 4s2 3d7 is the electron configuration for ___________ which has _________ electrons in its valence shell.
Answer: cobalt; 2
Q: You drive to Canada one day. Before you return you need to fill up with gas. However, the gas is sold per liter. If it takes 88.74 liters. How many gallons did you need to fill the car.1 liter – 1.06 quarts1 gallon = 4 quarts
Answer: 23.52 gallons
Q: Express 42004.3 x 1012 in proper scientific notation
Answer: 4.20043 x 1016
Q: A sample of iron with a mass of 4.50 pounds must be converted to milligrams. The answer is:(1kg = 2.2046 pounds; 1kg = 1000g;;1g = 1000 mg)
Answer: 2.04 x 10^6 mg
Q: You are asked to determine the mass required for an object. It displaces 49.6 ml of water when submerged and has a density of 0.85 g/ml.
Answer: 4.2 x 10^1 grams
Q: 40- An element has 17 protons, 17 electrons, 19 neutrons. Which element is described.
Answer: Chlorine
Q: Halogens will form a _________ charge in an ionic compound.
Answer: -1
Q: How many orbitals will be full if I have a d-subshell with 6 electrons
Answer: 1
Q: What subshell fills after the 4s subshell?
Answer: 3d
Q: Group IA elements are filling which subshell?
Answer: s
Q: Exam 2
Answer: Exam 2
Q: The Lewis symbol for Ca (calcium) will have ________ _______ (of) dot(s) representing electrons.
Answer: 2; single
Q: Elements in the Representative elements Group VA will have _________ valence electrons.
Answer: 5
Q: Typically, the maximum number of valence electrons for any element is __________
Answer: 8
Q: The ________ ________ follows that atoms of elements lose, gain, or share electrons in such a way as to produce a noble-gas electron configuration for each of the atoms involved.
Answer: Octet Rule
Q: 5-When an atom is electrically charged and loses an electron it is called a cation. Cations will have a ________charge.
Answer: Positive
Q: Sodium with a +1 charge will have a total of ________ electrons and ___________ protons.
Answer: 10; 11
Q: In aluminum fluoride (AlF_3 3 ) it is the aluminum that will __________ ________ electrons
Answer: lose; 3
Q: What is the chemical formula for the compound formed when Pb 4+ and O 2- ions interact.
Answer: PbO2
Q: The formula unit for NaCl is the number of atoms required to make it electrically ____________.
Answer: Neutral
Q: 10-Name MnO2
Answer: Manganese (IV) oxide
Q: What is the charge for the magnesium found in Mg(NO3)2
Answer: +2
Q: Neon (Ne) and Magnesium +2 ion (Mg 2+ ) are isoelectronic species. Another member of this category would be:
Answer: Sodium +1 ion
Q: A(n) ____________ bond results from two nuclei attracting the same shared electrons.
Answer: Covalent
Q: In Carbon dioxide CO2 there are ____________ pairs of bonding electrons.
Answer: 4
Q: 15-A covalent bond in which two atoms share three pairs of electrons is termed a(n) __________ bond
Answer: Triple
Q: A covalent bond in which both electrons of a shared pair come from one of the two atoms involved in the bond describes a ______________ covalent bond.
Answer: Coordinate
Q: In water, H2O, there are ________ bonding electron pairs and ________ non-bonding electrons pairs.
Answer: 2; 2
Q: The shape for the water molecule, H2O, is __________.
Answer: Angular
Q: How many VSEPR electron groups does CO2 have?
Answer: 2
Q: 20-How many VSEPR electron groups does HCN have?
Answer: 2
Q: What is the bond angle between the atoms of SO2
Answer: 120 degrees
Q: How many VSEPR electron groups does SO2 have?
Answer: 3
Q: What is the shape for NH3?
Answer: Trigonal pyramidal
Q: Fluorine(F) is _______ electronegative than Boron (B)
Answer: More
Q: 25-The bond between atoms in N2 is a(n)_________ covalent bond.
Answer: Non-polar
Q: The bond in HCl is _________. The chlorine has a partial ________ charge.
Answer: polar; negative
Q: Because H2S has a(n) _________ shape there is ______ and thus it is a ________ molecule.
Answer: angular; non-symmetry; polar
Q: What is the name for P2O3
Answer: diphosphorus trioxide
Q: How many atoms are in 1 mole of carbon?
Answer: 6.02 x 1023
Q: 30-What is the molar mass for CO2
Answer: 44.01 g per mole
Q: Calculate the mass of 2.50 moles of Carbon Monoxide, CO.
Answer: 70.0 grams of CO
Q: Calculate the number of moles in 50.0 grams of oxygen, O2
Answer: 1.56 moles of oxygen gas
Q: How many moles of oxygen atoms are present in 3 moles of C6H12O6
Answer: 18 moles
Q: How many Zinc (Zn) atoms are in a 100.0 gram sample of Zn?
Answer: 9.208 x 10 23
Q: 35-Balance the following equation: __C2H5OH + __O2 –> __CO2 +__H20
Answer: 1; 3; 2; 3
Q: Balance the following equation:___H20 –> ___H2 + ___O2
Answer: 2; 2; 1
Q: If you have 17.0 grams of NH3 and unlimited oxygen how many grams of water will be formed. Use the equation:4 NH3 + 5 O2 –> 4 NO + 6 H20 (balanced)
Answer: 27.0 grams of H20
Q: Particles are in constant random motion and possess ___________ energy.
Answer: kinetic
Q: The velocity of particles _______ as the temperature increases
Answer: increases
Q: 40-Particles in a system transfer energy to each other through __________ collisions.
Answer: elastic
Q: In a solid the _________ forces out weigh the ________ forces.
Answer: attractive; disruptive
Q: _____________ is the __________ applied per unit area on an object.
Answer: Pressure; force
Q: Convert 1.00 atmosphere into pounds per square inch
Answer: 14.7 psi
Q: Boyle’s law relates that ________ and ___________ are _____________ related when there is a constant temperature and number of moles.
Answer: pressure; volume; inversely
Q: 45-A sample of oxygen gas (O2) occupies 22.4 L at 23 degrees Celsius and 1.00 atm. What volume will it occupy at 3.00 atm when the temperature is constant.
Answer: 7.47 L
Q: In Charles’s Law ________ and Kelvin Temperature are ___________ related.
Answer: volume; directly
Q: A balloon containing 2.00 liters of air at 28.0 degrees cilsius is placed in a beak of liquid nitrogen at -78.5 degrees celsius. What will the volume of air become. (pressure is constant).
Answer: 1.29 liters
Q: At what pressure does 121 ml of O2 at 28 degrees celsius and 2.01 atm occupy a volume of 401 ml at 51 degrees celsius.
Answer: 6.53 x 10 -1 atm
Q: The pressure of the atmosphere is 760 torr. The pN2 is 600.4 torr. If oxygen is the only other gas what is the pO2?
Answer: 159.6 torr
Q: 50-Melting is a(n) ________________ change of state
Answer: Endothermic
Q: Water is boiling at the atmospheric pressure of 701 torr. What is its vapor pressure?
Answer: 701 mm Hg
Q: Hydrogen bonding will occur between F, _______, and N
Answer: Oxygen
Q: Chemistry Final
Answer: Chemistry Final.
Q: Anything that has mass and occupies space is?
Answer: Matter
Q: Choose the item that is NOT energy.
Answer: electrical wire
Q: Choose the homogenous mixture.
Answer: one visibly distinct phase
Q: A(n) ___________________ is a pure substance that can be broken down into two or more simpler pure substance by chemical means. For example, H20 or CO2 or NaCl
Answer: Compound
Q: Choose the proper chemical symbol for an element.
Answer: O
Q: Which is a triatomic molecule and a homeoatomic molecule?
Answer: O3
Q: How many atoms are in the formula (NH4)2MnO4
Answer: 15
Q: Which metric system prefix and base unit is the greater mass?
Answer: decigram
Q: Which has the most significant figures.
Answer: 14.0000000080000000000
Q: How many significant figures will the following problem’s answer be? 15.003000 x 2.90001 x 3 x 12.3
Answer: 1
Q: What is the answer with the correct number of significant figures for the following problem: 2334.445 + 7.83
Answer: 2342.28
Q: What is the expanded number for 3.920 x 10 -4
Answer: 0.0003920
Q: Convert the mass of a man that weighs 804 pounds into kilograms. 1.00 pound = 454 grams
Answer: 365 kg
Q: Convert 212 degree F into Kelvin
Answer: 373 K
Q: Electrons are found in the nucleus?
Answer: False
Q: Neutrons have a positive charge.
Answer: False
Q: Carbon-14 and Carbon-12 by both have an atomic number of ______ are considered to be ___________ and carbon-14 has ____ neutrons than carbon-12.
Answer: 6; isotopes; 2 more
Q: The element has 20 protons and 21 neutrons. What is the mass number for this element? What is the element named?
Answer: 41; Ca
Q: What is the group number for the Halogens?
Answer: VIIA
Q: What is the electronic configuration of potassium (K)?
Answer: 1s22s22p63s23p64s1
Q: How many valence shell electrons are represented in the following configuration: 1s22s22p63s23p64s23d4
Answer: 2
Q: Convert 1.204 x 1024 atoms of H2O into grams of H2O. Round to two significant figures.
Answer: 36 grams
Q: How many single dots should be surrounding nitrogen as a lewis symbol?
Answer: 3
Q: In a chemical reaction of Ca + Cl2 —-> CaCl2 what will be the charge on the calcium (Ca)? Is it a cation or an anion?
Answer: +2; cation
Q: Determine the proper chemical formula that results when Pb 4+ and O 2- form an ionic bond.
Answer: PbO2
Q: Name MgBr2
Answer: Magnesium bromide
Q: How many covalent bonds will N2 have?
Answer: Three
Q: How many VSEPR groups surround the central Carbon atom in hydrogen cyanide (HCN).
Answer: 2
Q: What is the shape for the molecule of SO2
Answer: Angular
Q: How many VSEPR groups surround the Sulfur (S) in the molecule of SO2 ?
Answer: 3
Q: Which atom is the most electronegative? O (oxygen), B (boron), C (carbon)
Answer: O
Q: Hydrogen Cyanide (HCN) is:
Answer: Polar
Q: A sample of hydrogen gas occupies 12.4 L at 23.0 degrees C and 0.056 atm. What volume will it occupy at 1.20 atm assuming that the temperature stays constant?
Answer: .58 L
Q: A balloon that has 1.30 L of Helium at 24.7 degree C is placed in a beaker containing liquid nitrogen at -78.5 degrees C. The volume will?
Answer: decrease
Q: What is the partial pressure of Nitrogen in the atmosphere when there is 79% Nitrogen gas and 21% oxygen at sea level pressures of 760 torr.
Answer: 600. torr
Q: At what pressure will water boil when atmospheric pressure is equal to 240 mm Hg?
Answer: 240 torr
Q: 20 grams of Sugar is dissolved in 1 Liter water. Which is correct?
Answer: sugar is the solute
Q: ____________ law described how gases will dissolve in a liquid at a given temperature according to the partial pressure. This law is useful in explaining the scuba diving phenomenon called the Bends.
Answer: Henry’s
Q: What is the percent by mass (m/m) of a solution that is composed of 12.0 grams sugar and 42.0 grams of water?
Answer: 22.2% (m/m)
Q: What is the Molarity (M) when 2.00 moles of sugar is dissolved in water and the volume is brought up to a total of 0.200 liter?
Answer: 10.0 M
Q: What is the Osmolarity of 14.0 Molar (M) solution of CaCl2
Answer: 42.0 M
Q: 2H2O → 2H2 + O2 is an example of a _______________ reaction
Answer: decomposition
Q: What is the oxidation number for Cr in the formula of K2Cr2O7
Answer: +6
Q: Zn(s) + 2HCl(aq) —>ZnCl2(aq) + H2(g) Which chemicals were oxidized? Zn or HCl? What was the oxidation state for Cl when it was paired with H in HCl
Answer: Zn; -1
Q: H2O(g) + CO(g) <==> H2(g) + CO2(g) For this equation the Keq is 1 x 10-30 With this Keq will there be more water or CO2 when the reaction reaches equilibrium.
Answer: More H2O
Q: A Bronsted-Lowry acid will _________ a proton.
Answer: donate
Q: NaOH will undergo _____________ in water. Because _____________ is the production of ions from a molecular compound that has been dissolved in solution.
Answer: dissociation; ionization
Q: H2SO4 is a(n) ____________ and will _________ two protons.
Answer: acid; donate
Q: A strong acid will donate _______ of its __________ ions
Answer: 100%; hydrogen
Q: What is the pH for a 1.0 x 10-4 M solution of OH- ions.
Answer: pH 10
Q: A pH of 12 is?
Answer: Basic
Q: The salt of a strong acid and a weak base will hydrolyze to give a pH
Answer: less than 7
Q: In nuclear chemistry an atom with a specific atomic number and a specific mass number is called a(n)?
Answer: Nuclide
Q: The most dangerous form of radiation is the _______ radiation.
Answer: gamma
Q: An alpha particle decay will release a(n)?
Answer: helium
Q: What is the value for X and Y in equation for radioactive decay that release a beta particle.\frac{234}{90}\text{Th}\:–>\:\:\frac{X}{Y}\text{Pa}\:\:+\:\frac{0}{-1}e
Answer: X is 234; Y is 91
Q: How many half-lives are required to bring 80 mg of Iodine-131 to 10 mg.
Answer: 3
Q: Which is a chemical change?
Answer: combusting propane
Q: Which is more likely to be a gas at a lower temperature? Polar H20 or non-polar CH4 at
Answer: Non-polar CH4
Q: Balance the following equation: KClO3 —> KCl + O2The coefficients should be
Answer: 2, 2, 3
Q: Convert 15 moles of NaCl to grams. Round to 2 significant figures.
Answer: 8.8 x 102 grams