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CHEM-112 WEEK 11-20
Which of the following atoms has the greatest number of unpaired electrons?
A: Cr
Which one of the following statements about orbitals is incorrect?
A: orbitals can hold two electrons provided they are spinning in the same direction
This type of wave has certain allowable states or energies.
A: standing
Which one of the following statements about d orbitals is incorrect?
A: d orbitals are filled before p orbitals in the same principal energy level
Electrons enter the 4s sub-level before the 3d sub-level because...
A: the 4s orbital has a lower energy
Quantum number that describes the average distance of the orbital from the nucleus.
A: principal
How many valence electrons does an electrically neutral atom of lead have?
A: 4
Which one of the following statements about s orbitals is incorrect?
A: they can only hold one electron
Smaller units that make up the sub-atomic particles of the nucleus.
A: Quarks
What alternative term do you use to refer to electron clouds or the probable path of electrons.
A: orbital
Which one of the following is not the electronic configuration of atom of a noble gas?
A: 1s22s2
Which element does not form chemical bonds more easily: gallium or nihonium?
A: nihonium
What is the classification of orbitals when they have the same energy?
A: degenerate
What is the electronic configuration of a sodium ion Na+?
A: 1s22s22p6
What is the electronic configuration of an oxide ion O2-?
A: 1s22s22p6
Higher electronegativity: niobium or tin?
A: tin
Another term for electron clouds or the approximate path followed by electrons.
A: orbital
Principle that states that it is impossible to know the exact position and momentum of an electron at
the same time.
A: uncertainty principle
Which one of the following is not isoelectronic with the others?
A: Mg+ - wrong/ Ne – wrong/ F- wrong/ Na- wrong / Mg & Ne – wrong/ Mg & Na – wrong/ Mg & F –
wrong/ F & Na – wrong/ F & Ne – wrong/ Ne & Na – wrong/ Na, Ne, F – wrong/ Na, F, Mg – wrong/
Mg, F, Ne – wrong/ Mg, Na, Ne – wrong/ Mg, Na, Ne, F – wrong
This quantum number gives you an idea on the shape of the electron orbital.
A: angular momentum
Number of energy levels in an atom of tungsten
A: 6
Which element has a larger atom: technetium or gold?
A: gold
Which element forms chemical bond more easily: rutherfordium or flerovium?
A: flerovium
(2 points) A hydrogen electron moves with a velocity of 2.2 x 106 m/s in its ground state energy
level. What is the de Broglie wavelength of this particle? x 10-10 m
A: 3.3
Which statement about copper is incorrect?
A: the electronic configuration of copper atoms is 1s22s22p63s23p64s23d9
This states that it is impossible to know where and how fast an electron is at the same time.
A: uncertainty principle
Which element requires more energy to release an electron: copper or roentgenium?
A: copper
Which of the atom pairs both have only three unpaired electrons in their d orbitals?
A: V and Co
This quantum number describes how the direction of the electron along its orbit.
A: spin
Particle that is approximately as heavy as a proton but is neutrally charged.
A: neutron
An atom of meitnerium has how many energy levels?
A: 7
Which one of the following ions has an electronic configuration similar to argon?
A: Ti4+
The electronic configuration of an atom an element with atomic number 8 is...
A: 1s22s22p4
This is the basis of the assumption that electrons are added to an atom starting with the lowest
energy orbital.
A: Aufbau principle
The order of filling orbitals is...
A: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p
How many energy levels does an atom of plutonium have?
A: 7
How many valence electrons does an electrically neutral atom of thallium have?
A: 3
Number of valence electrons in an electrically neutral atom of antimony
A: 5
Lower ionization energy: sulfur or polonium?
A: polonium
Which element more easily releases an electron: technetium or indium?
A: indium
Which one of the following statements about p orbitals is incorrect?
A: they are found in all principal energy levels
What is the absolute value of the possible values for the spin quantum number of an electron?
A: ½
Higher atomic radius: chlorine or osmium?
A: osmium
Which element has a smaller atom: zirconium or tellurium?
A: tellurium
Type of ion to be formed by tin.
A: anion
Which of the following is a salt?
A: zinc selenide
Which of these compounds can conduct electricity when mixed with a solvent?
A: Lithium oxide
Type of ion assumed by a non-metal.
A: anion
Form of atom that forms ionic bonds.
A: ions
Type of ion to be formed by antimony.
A: anion
What element is the anion in sodium selenide?
A: selenium
Which among these compounds will boil first?
A: Chlorine trifluoride
Type of ion to be formed by potassium.
A: cation
Which of these compounds has weaker bonds between its component atoms?
A: Arsenic trioxide
Bond formed between a metal and a non-metal.
A: ionic
Which of the following is not a salt?
A: iodine trichloride
Which of these compounds will relatively melt first?
A: Bromine pentafluoride
What element is the cation in potassium oxide?
A: Potassium
Which of these compounds is more difficult to boil?
A: Barium Selenide
Type of ion to be formed by magnesium.
A: cation
Which of the following is not a salt?
A: carbon tetrachloride
Happens to electrons that results to formation of ionic bonds.
A: transfer
Which of these compounds can exist only in solid form?
A: Barium iodide
Which of these compounds will relatively melt last?
A: Potassium bromide
What element is the cation in sodium fluoride?
A: sodium
What element is the cation in calcium chloride?
A: calcium
What element is the anion in silver oxide?
A: oxygen
Which of these compounds has a relatively high melting point?
A: Sodium bromide
Type of ion assumed by a metal.
A: cation
Which of the following is a salt?
A: zinc fluoride
Which of these compounds can never conduct electricity even in aqueous solution?
A: Dioxygen difluoride
Happens to electrons in ionic bonding.
A: transferred
Which of these compounds has stronger bonds between its atom components?
A: Potassium chloride
All of the following compounds (in solid form) are hard EXCEPT for…
A: Ethanol
How many covalent bonds can an atom of oxygen form?
A: 6
How many dots should be around a neutral atom of tennessine?
A: 7
What type of bond can form between nitrogen and hydrogen?
A: covalent
Shows the number of valence electrons of an atom in a Lewis representation.
A: dot
Number of lone pairs around the central atom in the bent geometry of a polar compound.
A: 2
What kind of compound is chlorine trifluoride?
A: Covalent
Which element is more electronegative: tin or antimony?
A: antimony
When formed as a compound, in which of these two elements will there be more electrons:
germanium or phosphorous?
A: phosphorous
What is the geometry of the non-polar covalent compound with no lone pairs around the central
atom but has three bonding electron groups it?
A: Trigonal planar
Manner of bonding between two non-metals.
A: sharing
Kind of compound with one side positive and the other negative.
A: polar
Tendency of an atom to attract electrons in a bond.
A: electronegativity
Which of the following compounds is a good conductor of electricity when in a solution?
A: Potassium nitride
What is the bonding mechanism in ammonium sulfide?
A: transfer of electrons
Geometry of polar compound with one lone pair around the central atom.
A: pyramidal
Which of these two elements will attract electrons more than the other: nihonium or oxygen?
A: oxygen
Number of maximum valence electrons an atom can have.
A: 8
Observed in determining how many bonds an atom can have.
A: Octet rule
Which of the following molecules does not involve sharing of molecules?
A: zinc selenide
Identify which of the following compounds with boil first when heated.
A: Chlorine trifluoride
Type of bonding between molecules wherein the electrons are shared.
A: Covalent
Which compound can serve as a good insulator?
A: ozone
Representation of the number of valence electrons of the atom of an element.
A: all of the choices are correct
Which of the following is not a covalent compound?
A: zinc fluoride
What type of bond will possibly form between carbon and potassium?
A: Ionic
Which of the following is a covalent compound?
A: carbon tetrachloride
Which of the following has covalent bonds in it?
A: iodine trichloride
Identify the compound that will easily dissolve in water.
A: Zinc phosphate
Which of the following compounds melts first when subjected to the same amount of heat?
A: Carbon monoxide
What element is the anion in barium sulfide?
A: Sulfur
Identify the following compounds if they are ionic or covalent:
Fe2O3
A: Ionic
The ability of an atom to attract electrons in the presence of another atom is a measurable property
called
A: electronegativity
A set of covalently bonded atoms that have an overall charge, making them an ion.
A: Polyatomic ion
A carbon atom has fix electrons, four of which are in the outer shell of the atom, its valence shell.
A: true
It is an ion with more electrons than protons giving it a net negative charge.
A: anion
Different compounds that have the same molecular formula.
A: isomers
It is a change in the chemical bonds of one or more molecules.
A: Chemical reaction
Although each isotope has varying numbers of neutrons, there is difference to the chemical
reactions of the carbon atom.
A: false
It is a substance made by combining two or more different materials in a such a way that no
chemical reaction occurs.
A: mixture
What do you call two monomers that are connected?
A: Dimer
Covalent bonding can be visualized with the aid of
A: Lewis diagram
They are organic molecules consisting entirely of carbon and hydrogen, such as methane (CH4)
A: Hydrocarbons
A type of chemical bond where two atoms are connected to each other by the sharing of two or more
electrons.
A: Covalent bond
A bond in which or more electrons from one atom are removed and attached to another atom
resulting in positive and negative ions which allow each other.
A: ionic bond
Organic acids that contain a carbon atom that participates in both a hydroxyl and a carbonyl
functional group.
A: Carboxylic acids
They are specific atoms, ions, or groups of atoms having consistent properties.
A: Functional groups
They are specific atoms, ions, or groups of atoms having consistent properties.
A: Functional groups
This functional group is produced from the condensation of an alcohol with a carboxylic acid and is
named based on these components.
A: Esters
It is a natural component of crude oil and has been classified as a carcinogen.
A: bezene
These are compounds with a nitrogen atom, a lone pair of electrons, and three substituents.
A: aminos
Class of organic compounds characterized by an oxygen atom connected to two alkyl or aryl groups.
A: esters
It is the simplest hydrocarbon molecule, with a central carbon atom bond to form different hydrogen
atoms.
A: methane
This is a model that is based on the repulsive behaviour of electron-pairs.
A: VSEPR
They are formed by successive bonds between carbon atoms and may be branched or unbranched.
A: Hydrocarbon chains
It contains a carbon-carbon double bond.
A: alkenes
Having a closed ring of alternate single and double bonds with delocalized electrons.
A: Aromatic chain
Carbon atoms have six protons in the nucleus and six electrons orbiting around the nucleus.
A: true
Carbon compounds containing boron and silicon are among the hardest substances known.
A: true
Monomers covalently bonded to one another in longer chains.
A: polymers
They are organic molecules consisting entirely of carbon and hydrogen, such as methane (CH4).
A: Hydrocarbons
It refers to a specific group of atoms bonded in a certain arrangement that give a compound certain
physical and chemical properties.
A: Functional groups
A smaller organic molecule that often plays its own functional roles in living organisms.
A: monomer
Identify the following compounds if they are ionic or covalent:
C4
A: Covalent
Identify the following compounds if they are ionic or covalent:
H2O
A: Covalent
The basic geometry for a molecule containing a central atom with three pairs.
A: trigonal planar
They are classes of organic compounds that contain a carbonyl (C=0) group.
A: Aldehydes and ketones
A class of organic compounds in which the carbon atoms are arranged in an open chain.
A: Aliphatic
It is present in many biological molecules including some amino acids and most steroids, which
includes cholesterol and the hormones estrogen and testosterone.
A: Benzene ring
In this type of reaction, a water molecule is released as a product, effectively dehydrating the
reactants as a larger biomolecule is synthesized.
A: Dehydration synthesis
Identify the following compounds if they are ionic or covalent:
KNO3
A: ionic
Identify the following compounds if they are ionic or covalent:
CH4
A: covalent
The most electronegative element
A: Fluorine
It is a dark grey crystalline solid with a purple vapour. It is very slight with soluble in water, but
dissolve freely in organic solvents.
A: Iodine
They are highly acidic and almost exclusively existing in an ionized state in solutions by releasing
two hydrogen ions.
A: phosphates
Carbon compounds come in the form of diamond graphite, charcoal, carbon block and fullerene.
A: true
Functional groups characterized by the presence of an “OH” group.
A: Alcohols
Reactions incorporate the atoms from a water molecule into each monomer as the chemical bond
between the monomers is broken.
A: Hydrolysis
An organic compound that consist of a carbon bonded to an OH group
A: propanol
The building blocks of proteins
A: AMINO ACIDS
Carbon double bonded to oxygen
A: CARBONYL GROUP
The electron cloud is divided into 7 principal energy levels numbered n=1 to n=7 with n=1 closest to
nucleus. n is called
A: principal quantum number
Name the compound.
SiF4
A: Silicon tetrafluoride
Name the compound. BeI2
A: Beryllium iodide
This describes the wavelike behaviour of either one electron or a pair of electrons in an atom.
A: ATOMIC ORBITAL
Name the compound. HF
A: hydrogen monofluoride
Lipid molecules hold a large amount of energy and are energy storage molecules.
A: TRUE
What are the atoms that have to pair to form these given chemical formulas?
KF= Potassium+fluorine
MgI2= Magnesium+iodine
AlCl3= Aluminum+chlorine
CaCl2= Calcium+chlorine
Na2O= Sodium+Oxygen
They carry genetic information in the cell. They also help in synthesis of proteins, through the
process of translation and transcription.
A: Deoxyribonucleic acids
It is a type of chemical bond where a pair of electrons is unequally shared between two atoms
A: POLAR COVALENT BOND
The ionization energy of the elements within a group generally increases from top to bottom. This is
due to electron shielding.
A: FALSE
A compound that contains COO
A: Carboxylic acid
It is found in many different compounds. It is the sixth most abundant element in the universe.
A: CARBON
This type of compound always contains the carbon atom.
A: ORGANIC
The higher the energy is, the more readily the atom becomes a cation.
A: FALSE
Determine if the elements in the following compounds are metals or non-metals. Describe the type of
bonding that occurs in the compound.
SO2 Non-metal Non-metal Ionic
MgBr2 Metal Non-metal Covalent
CaO Metal Non-metal Ionic
H2O Non-metal Non-metal Covalent
Cu - Zn alloy Metal Metal Metallic
Name the compound.K2O
A: Potassium oxide
Electronegativity is a qualitative property and there is standardized method for calculating
electronegativity.
A: false
When a protein in an assembly of more than one polypeptide or subunits of its own, this is said to be
the structure of protein that is categorized as
A: Quarternary
A carboxylic acid that has a long hydrocarbon chain and derived from a natural source.
A: Fatty acid
It is a large molecule or macromolecule, composed of many repeated subunits, that is not artificially
manufactured.
A: Natural Polymer
Basic component that makes up any kind of material.
A: atom
This basically makes up any kind of material
A: atom
Anything that occupies space and has mass
A: matter
What is the general term for any body that has mass and occupies space?
A: matter
General term referring to anything that occupies space and has mass
A: matter
Study of materials and its components
A: Chemistry
General term for anything with mass and has volume
A: matter
Quantities standardized for scientific use.
A: SI
Smallest building block of any material
A: atom
Branch of chemistry that deals with compounds containing carbon
A: organic
Path of electron around the nucleus of an atom
A: orbit
Most basic building block of any substance
A: atom
Quantity with square unit
A: pressure
What kind of base forms hydroxide ions when mixed with water?
A: weak
Path followed by an electron around the nucleus of an atom
A: orbit
What do you call the path of an electron around the nucleus of an atom?
A: orbit
Science that deals with the chemical composition of chemical processes associated with the Earth
and other planets.
A: geochemistry
Reaction involved when a complex reactant is broken down into a simpler product.
A: decomposition
What kind of reaction is involved when a complex reactant is simplified?
A: decomposition
Science dealing with the composition of processes involving the Earth and other planets
A: geochemistry
Quantity that refers to the space occupied by a body
A: volume
Quantity referring to the space occupied by a body
A: volume
Gas law involving constant pressure.
A: charle’s law
Product of the combination of atoms during chemical reactions
A: molecule
Results from the combination of atoms during chemical reactions
A: molecule
What substance results from the combination of atoms during chemical reactions?
A: molecule
Term used to refer to a charged atom
A: ion
In one molecule of water, how many percent is hydrogen?
A: 11.19
Consider one molecule of water. How many percent of this molecule is hydrogen?
A: 11.19
In the oxidation of methane alcohol in air, if 209 grams of this substance are used up, how many
grams of water are produced?
A: 235
How heavy (in grams) is one molecule of ethanol
A: 46.07
Consider the burning of methanol in air. If 209 grams of methanol are used up in the combustion,
how much water (in grams) is produced?
A: 235
What is the chemical reaction characterized by the union of reactants
A: synthesis
What is the chemical reaction characterized by the union of reactants?
A: synthesis
How heavy is a molecule of sodium hypochlorite? Express your answer in grams.
A: 74.44
How heavy (in grams) is one molecule of sodium hypochlorite?
A: 74.44
When burning 1200 grams of carbon, how much carbon monoxide (in grams) will be produced?
A: 2800
In the burning of 1200 grams of carbon, how many grams of carbon monoxide will be produced?
A: 2800
When 124 grams of aluminum reacts with 601 grams of Fe2O3, determine how many grams of
Al2O3 are formed.
A: 234
How many molecules are in 3 moles of calcium tetrachloride?
A: 1.8066 x 10^24
In a molecule of ammonia, how many percent is nitrogen?
A: 82.24
Consider a molecule of ammonia. How many percent of this molecule is nitrogen?
A: 82.24
How heavy (in grams) is one molecule of ethanol?
A: 46.07
Consider a molecule of ethane. How many percent of ethane is carbon?
A: 79.89
In one molecule of ethane, how many percent of this molecule is carbon?
A: 79.89
In a molecule of potassium hydroxide, how many percent of this molecule is oxygen?
A: 28.52
The molecular mass of hydrochloric acid is how many grams?
A: 36.46
The mass of hydrochloric acid is how many grams?
A: 36.46
How many grams is a molecule of hydrochloric acid?
A: 36.46
How heavy is a molecule of sodium hypochlorite? Express your answer in grams
A: 74.44
How many molecules are there in 8 moles of benzoic acid?
A: 4.8176 x 10^24
Consider the reaction of 124 grams of Al with 601 grams of Fe2O3. Compute for the mass (in
grams) of Al2O3 formed.
A: 234
Consider one molecule of sodium sulfate. Determine the percentage of sulfur in it.
A: 22.57
In a molecule of sodium sulfate, determine the percentage of sulfur in it.
A: 22.57
In one molecule of sodium sulfate, how many percent of it is sulfur?
A: 22.57
How many molecules are there in 0.75 mole of sodium chloride?
A: 4.5165 x 10^23
A 0.75 mole of sodium chloride has ___ x 1023 atoms. Note: The answer must be in 4 decimal
places.
A: 4.5165
Find the molecular mass of hydrogen peroxide in grams?
A: 34.01
What is the molecular mass (in grams) of hydrogen peroxide?
A: 34.01
Determine the molecular mass (in grams) of dinitrogen trioxide?
A: 76.01
What is the molecular mass (in grams) of dinitrogen trioxide?
A: 76.01
How heavy (in grams) is one molecule of ethanol?
A: 46.07
How many grams is one molecule of ethanol?
A: 46.07
Suppose you want to burn 1200 grams of graphite. How much oxygen (in grams) would you need?
A: 1600
If you want to burn 1200 grams of carbon, how many grams of oxygen would you need?
A: 1600
How many grams is one molecule of calcium oxide?
A: 56.08
How heavy (in grams) is calcium oxide?
A: 56.08
How heavy (in grams) is one molecule of sulfuric acid?
A: 98.07
How many grams is a molecule of sulfuric acid?
A: 98.07
What is the mass (in grams) of sulfuric acid?
A: 98.07
Determine how many atoms of carbon dioxide does 0.55 mole of this molecule has? ____ x 1021
A: 7.53
A 0.55 mole of carbon dioxide has ___ x 1021 atoms.
A: 7.53
How many molecules does 0.55 mole of carbon monoxide has?
A: 7.53 x 10^21
What do you call the particle with more positive charges than negative charges?
A: cation
What is the molecular mass (in grams) of calcium carbonate?
A: 162.11
What do you call the agent in a redox reaction from which electrons are released?
A: reducing
Agent in a redox reaction from which electrons are removed.
A: reducing
The twelve-gauge copper wire is roughly cylindrical and has a diameter of approximately 0.1040 in.
The density of copper is 8.92 g/cm3 and copper atoms have an approximate atomic radius of 135
pm. What is the mass (in grams) of a 100-ft piece of copper wire?
A: 1491
Quantity used to measure distance between two points.
A: length
Quantity that measures the distance between two bodies
A: length
Made up of proton/s, neutron/s, and electron/s.
A: atom
Composed of proton/s, neutron/s, and electron/s
A: atom
This body is composed of proton/s, neutron/s, and electron/s.
A: atom
Which of the following is the lightest particle?
A: electron
Term used to refer to a charged atom.
A: ion
Which is the lightest: proton, neutron, or electron?
A: electron
Particle that contains more positive charges than negative charges.
A: cation
Particle with more positive charges than negative charges
A: cation
Science that deals with the composition of materials.
A: chemistry
Study dealing with the composition of materials
A: chemistry
What kind of acid completely dissociates when mixed with water?
A: strong
Composed of a nucleus and electron/s.
A: atom
Always has a nucleus and electron/s
A: atom
Science that deals with energy and its interactions with matter.
A: physics
Science of energy and its interactions with different materials
A: physics
Particle with more negative charges than positive ones.
A: anion
Particle having more negative charges than positive ones
A: anion
Type of bond between a cation and an anion.
A: ionic
Form of atom that is positively charged with respect to its neutral state.
A: cation
What type of bond exists between a cation and an anion?
A: ionic
Atom with a positive charge with respect to its neutral state
A: cation
Chemistry that deals with compounds with carbon
A: organic
What quantity is constant in Charles's law?
A: pressure
Formed when atoms combine through bonds.
A: molecule
How many grams is one molecule of sodium bicarbonate?
A: 84.01
What is the mass (in grams) of sodium bicarbonate?
A: 84.01
Amount of material contained by a body.
A: mass
Measurement of the amount of material in a body
A: mass
This refers to the amount of material in any given body.
A: mass
An atom that is negatively charged.
A: anion
Negatively-charged atom
A: anion
Chemistry of materials related to living tissues.
A: biochemistry
Chemistry living tissues.
A: biochemistry
This branch of chemistry is related to living tissues.
A: biochemistry
Method of comparing an unknown quantity with a known quantity
A: measurement
Process of comparing an unknown quantity with a known quantity.
A: measurement
Bond formed by the sharing of electrons between atoms.
A: covalent
Bond formed through the sharing of electrons between atoms
A: covalent
What kind of bond is formed by the sharing of electrons between atoms?
A: covalent
Comparison of something unknown with a standard.
A: measurement
Quantity used to express the amount of a substance.
A: mole
What is the percentage of hydrogen in propanoic acid?
A: 8.16
How many percent of propanoic acid is hydrogen?
A: 8.16
Quantity expressed with cubic unit.
A: volume
Three moles of methane has ____ x 1024 molecules.
A: 1.8066
Eight moles of benzene has ____ x 1024 molecules. Note: The answer must be in 4 decimal places.
A: 4.8176
Reaction wherein the anions and cations of two compounds switch places to form two entirely
different compounds.
A: double replacement
This reaction involves the anions and cations of two compounds switching places to form two
entirely different compounds.
A: double replacement
Uses Avogadro’s number to have a numerical value.
A: mole
Reaction that involves the transfer of protons from an acid to a base.
A: acid-base
Reaction characterized by production of a complex product from simple reactants.
A: synthesis
It is the phase in which the sister chromatid separate.
A: anaphase
What type of reaction is characterized by the production of a complex product from simple
reactants?
A: synthesis
How many percent of one molecule of potassium hydroxide is oxygen?
A: 28.52
How much (in percent) of one molecule of potassium hydroxide is oxygen?
A: 28.52
This particle has more negative charges than positive ones.
A: anion
Reaction involved when a complex reactant is broken down into a simpler product.
A: (synthesis)
Reaction generally described as: AB + C AC + B
A: single replacement
This type of reaction is generally described as: AB + C -> AC + B
A: single replacement
What is the process of comparing an unknown quantity with a known quantity?
A: measurement
Chemical reaction characterized by the combination of reactants.
A: synthesis
How much volume (in L) will 0.20 mol hydrogen iodide at 300 K and 100.0 kPa occupy? Use R = 8.314
kPa*L/(K*mol) = 0.08205 atm*L/(mol*K).
A: 5
How many molecules are present in 3 moles of methanal?
A: 1.8066 x 10^24
Type of bond between an anion and a cation
A: ionic
In a titration experiment, 500 mL of gaseous hydrochloric acid at 300 K and 100 kPa dissolved in pure
water is needed to neutralize 12.5 mL of sodium hydroxide. What is the concentration of the basic
solution (in mol/L)?
A: 1.60
Substance formed when atoms bond with each other
A: molecule
Identify which quantity is constant in Boyle's law.
A: temperature
What is the resulting concentration (in mol/L) of aqueous hydrochloric acid if 500 mL of its gaseous form
at 300 K and 100 kPa will be dissolved in 100 mL pure water? Use 8.314 kPa*L/(K*mol).
A: 0.200
Consider the reaction of 3.66 g of a sample containing zinc (atomic weight = 65.4) and magnesium
(atomic weight = 24.3) with a dilute acid to yield 2.470 L of hydrogen gas at 101.0 kPa and 300 K. What is
the percentage of zinc in the sample?
A: 30
(2 points) Suppose 4 moles of nitrogen gas are confined to a 6.0 L container at 1770C and 12.0 atm.
If the container will be allowed to isothermally expand to 36.0 L, determine the final pressure
experienced by the gas. (Express the answer in atm)
A: 2
Gas law involving constant pressure and temperature.
A: avogadro’s law
Quantities specifically used in scientific measurements
A: SI
(2 points) A 60.0 liter tank of gaseous chlorine at 270C and 125 atm suddenly had a leak. When this
leak was discovered, the pressure was found to have reduced to 50 atm. Determine how many
moles of chlorine escaped from the tank.
A: 187.5
Consider 6.2 liters of an ideal gas compressed at 3.0 atm and maintained at 37 degrees Celsius.
Determine how many moles of this gas are contained.
A: 0.75
One liter of an air sample at 250 degrees Celsius and 1 atm is compressed to 3 mL at a pressure of
1000 atm. Determine the temperature of the air sample in kelvins.
A: 983
Gas law involving constant temperature.
A: Boyle's Law
Treating 50.0 mL of silver nitrate solution with excess hydrogen iodide gas produces 2.35 grams of silver
iodide. Compute for the concentration (in M) of the silver nitrate solution.
A: 0.2
(3 points) Suppose methanol will be burned in air. If 209 grams of this substance are used up in the
reaction, how many grams of water are produced?
A: 235
(2 points) Consider a 0.316 mole sample of nitrogen gas. If this is placed in a 4-L container at 315 K, what
is the pressure (in torr) of the gas?
A: 1550
The noble gases possess very high ionization energies because of their full valence shells.
A: TRUE
Electron affinity is a quantitative measurement of the energy change that occurs when an electron is
added to a neutral gas atom.
A: TRUE
Encircle the one that is not an example of polar compounds
A: Sulphur dioxide
This model of the atom uses complex shapes of orbitals, volumes of space in which there is likely to
be an electron. This model is based on probability rather than certainty.
A: Quantum mechanical model
They are atoms which have the same atomic number but different mass numbers.
A: isotopes
This type of polymer is derived from petroleum oil and made by scientists and engineers.
A: Synthetic
Ionization energy increases from left to right on the periodic table.
A: true
In Ionic bonds, the metal loses electrons to become a positively-charged cation, whereas the nonmetal accepts those electrons to become a negatively-charged ion.
A: true
The least electronegative atom and should be the central atom.
A: nitrogen
Name the compound.
SrO
A: Strontium oxide
This compound, usually formed by the dehydration-condensation reaction of an oxoacid, yields two
molecules of the acid when it reacts with water.
A: Acid anhydride
It is molecule that is present in living organisms, including large macromolecules such as proteins,
carbohydrates, lipids and nucleic acids, as well as small molecules such as primary metabolites
secondary metabolites and natural products.
A: Biomolecules
Electron shielding describes the ability of an atom’s inner electrons to shield its positively-charged
nucleus from its valence electrons.
A: true
In Ionic bonds, the metal loses electrons to become a positively-charged cation, whereas the nonmetal accepts those electrons to become a negatively-charged ion.
A: true
Periodic trends are specific patterns that are present in the periodic table that illustrate different
aspects of a certain element, including its size and its electronic property.
A: true