Chemistry MidTerm Review
Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius?
-34oC
What is the net charge of the ionic compound calcium fluoride? ᅞA: 2- ᅞB: 1- ᅚC: 0 ᅞD: 1+
0
How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound potassium nitride?
0 nitrogen electrons don't transfer
A train travels at a speed of 30 miles per hour. If 1 mile = 1.6 kilometers, how fast is the train traveling in kilometers per minute?
0.8 km/min
How many of the following molecules are polar? BrCl3 CS2 SiF4
1
How many pi bonds are formed when sp2 hybridization occurs in ethene, C2H4? ᅞA: 0 ᅚB: 1 ᅞC: 2 ᅞD: 3
1
In a pyramidal molecule, how many unshared pairs of valence electrons does the central atom have? ᅞA: none ᅚB: one ᅞC: two ᅞD: three
1
If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? 1. 20 10E 2. 20 11E 3. 21 9E 4. 21 10E
1 and 4
What is the charge on an alpha particle?
2+
What is the charge on the strontium ion? ᅞA: 2- ᅞB: 1- ᅞC: 1+ ᅚD: 2+
2+
In the measurement 0.503 L, which digit is the estimated digit?
3
5.5234 mL of mercury is transfered to a graduated cylinder with scale marks 0.1 mL apart. Which of the following will be the correct reading taken from the graduated cylinder?
5.52 mL always measure one more than the container has
What is the number of electrons in the outermost energy level of an oxygen atom?
6
Which of the following sets of symbols represents isotopes of the same element? ᅞA: 9142J 9242J 9340J ᅞB: 5019L 5020L 5021L ᅚC: 8438M 8638M 8738M ᅞD: 13859Q 13355Q 13354Q
8438M 8638M 8738M
Refers to how close a measured value is to an accepted value
: accuracy
Multiply the following three numbers and report your answer to the correct number of significant figures: 0.020 cm x 50 cm x 11.1 cm = ?
D: 11.1 cm3 three sig figs
Which isotope of Ruthenium (Ru, atomic number 44) has the greatest nuclear stability? A: Ru 100 ᅞB: Ru 102 ᅞC: Ru 101 ᅚD: Ru 104
D: Ru 104
Which of the following may have more than one phase? ᅞA: a pure solid ᅞB: a pure liquid ᅞC: a homogeneous mixture ᅚD: a heterogeneous mixture
D: a heterogeneous mixture
Brass is an alloy of
copper and zinc
When you decide whether or not the data supports the original hypothesis, you are
drawing conclusions
Which molecule has a single covalent bond? ᅞA: CO2 ᅚB: Cl2 ᅞC: CO ᅞD: N2
ᅚB: Cl2
Which group of measurements is the most precise? (Each group of measurements is for a different object.) ᅞA: 2 g, 3 g, 4 g ᅞB: 2.0 g, 3.0 g, 4.0 g ᅚC: 2 g, 2.5 g, 3 g ᅞD: 1 g, 3 g, 5 g
ᅚC: 2 g, 2.5 g, 3 g
What are the missing coefficients for the skeleton equation below? Cr(s) Fe(NO3)2(aq) Fe(s) Cr(NO3)3(aq) ᅞA: 4, 6, 6, 2 ᅞB: 2, 3, 2, 3 ᅚC: 2, 3, 3, 2 ᅞD: 1, 3, 3, 1
ᅚC: 2, 3, 3, 2
When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is ____. ᅞA: KH + BaCl --> KCl + BaH ᅞB: KOH + BaCl --> KCl + BaOH ᅚC: 2KOH + BaCl2 --> 2KCl + Ba(OH)2 ᅞD: KOH + BaCl2 --> KCl2 + BaOH
ᅚC: 2KOH + BaCl2 --> 2KCl + Ba(OH)2
The expression of 5008 km in scientific notation is
ᅚC: 5.008 E3 km
What is the result of multiplying 2.5 E 10 by 3.5 E -7 ?
ᅚC: 8.75 E3
Place the following in order of decreasing metallic character. C O N F ᅞA: O > N > F > C ᅞB: F > O > N > C ᅚC: C > N > O > F ᅞD: F > N > O > C ᅞE: N > C > O > F
ᅚC: C > N > O > F
The least electronegative element from among the following is ᅞA: Na. ᅞB: Cl. ᅚC: Cs. ᅞD: S.
ᅚC: Cs the smaller is the most electronegative
Choose the compound below that should have the lowest melting point according to the ionic bonding model. ᅞA: LiF ᅞB: NaCl ᅚC: CsI ᅞD: KBr ᅞE: RbI
ᅚC: CsI they are bigger , lower melting point
ho was the man who lived from 460 B.C.±B.C. and was among the first to suggest the idea of atoms? Atomos ᅞB: Dalton ᅚC: Democritus ᅞD: Thomson 1/
ᅚC: Democritus
Which of the following represents a compound? ᅞA: H ᅞB: <i>H-3</i> ᅚC: H<sub>2</sub>O ᅞᅞD: O-16
ᅚC: H<sub>2</sub>O
Identify the compound with the highest magnitude of lattice energy. ᅞA: NaCl ᅞB: KCl ᅚC: LiCl ᅞD: CsCl
ᅚC: LiCl the smaller the more lattice energy
Which of the following is the correct skeleton equation for the reaction that takes place when solid phosphorus combines with oxygen gas to form diphosphorus pentoxide? ᅞA: P(s) + O2(g) --> PO2(g) ᅞB: P(s) + O(g) --> P5O2(g) ᅚC: P(s) + O2(g) --> P2O5(s) ᅞD: P2O5(s) --> P2(s) + O2(g)
ᅚC: P(s) + O2(g) --> P2O5(s)
Which of the following is true about compounds? ᅞA: They can be physically separated into their component elements. ᅞB: They have compositions that vary. ᅚC: They are substances. ᅞD: They have properties similar to those of their component elements.
ᅚC: They are substances.
Of the following elements, which one has the smallest first ionization energy? ᅞA: boron ᅞB: carbon ᅚC: aluminum ᅞD: silicon
ᅚC: aluminum
Which of the following factors contributes to the increase in ionization energy from left to right across a period? ᅞA: an increase in the shielding effect ᅞB: an increase in the size of the nucleus ᅚC: an increase in the number of protons ᅞD: fewer electrons in the highest occupied energy level
ᅚC: an increase in the number of protons because there is more pull
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4. ᅞA: eg=tetrahedral, mg=tetrahedral ᅞB: eg=linear, eg=linear ᅞC: eg=tetrahedral, mg=bent ᅞD: eg=trigonal bipyramidal, mg=tetrahedral ᅚE: eg=octahedral, mg=square planar
ᅚE: eg=octahedral, mg=square planar
How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum? ᅞA: The speed of visible light is greater. ᅞB: The speed of gamma rays is greater. ᅚC: The speeds are the same. ᅞD: No answer can be determined from the information given.
ᅞA: The speed of visible light is greater
Which of the following combinations of symbol and explanation of symbol is correct when used in a chemical equation? ᅞA: (g), grams ᅞB: (l), liters ᅚC: (aq), dissolved in water ᅞD: (s), solid product
ᅞD: (s), solid product
The shape (not the size) of an electron cloud is determined by the electron's ____. ᅚA: energy sublevel ᅞB: position ᅞC: speed ᅞD: principal quantum number
ᅞD: principal quantum number
What are the missing coefficients for the skeleton equation below? Cr(s) + Fe(NO3)2(aq) --> Fe(s) + Cr(NO3)2(aq) ᅞA: 4, 6, 6, 2 ᅞB: 2, 3, 2, 3 ᅚC: 2, 3, 3, 2 ᅞD: 1, 3, 3, 1 ᅞE: 1, 1, 1, 1
ᅞE: 1, 1, 1, 1
Express the sum of 1111 km and 222 km using the correct number of significant digits.
1333 km
Which of the following electron configurations of outer sublevels is the most stable? ᅚA: 4d5 5s1 ᅞB: 4d4 5s2 ᅞC: 4d3 5s3 ᅞD: 4d2 5s4
4d5 5s1
Divide the following three numbers and report your answer to the correct number of significant figures: 0.530 g / 0.1010 mL = ?
5.248 g/mL 4 sig figs
Correctly rounded, the sum of 1.2 E-3 cm and 2.7 E-4 cm is
: 0.001 cm
Add the following three numbers and report your answer using significant figures: 2.5 cm + 0.50 cm + 0.055 cm =
: 3.1 cm
What is the formula unit of sodium nitride?
: Na3N
Iron has three isotopes. 5.84 % of iron is Fe-54, 91.68% of iron is Fe-56 and 0.31% of iron is Fe-58. Without doing any calculations, what is the approximate average atomic mass of iron
: about 56 amu look on periodic table
Research on solubility as a factor that affects the digestion of foods in humans would be an example of
: applied research
The number of neutrons in the nucleus of an atom determines the: ᅞA: the identity of the atom ᅞB: the atom's nuclear charge ᅚC: the nuclear stability of the atom ᅞD: the physical and chemical properties of the atom
: the nuclear stability of the atom
Which discovery did J. J. Thomson make that improved upon Dalton's atomic theory? ᅚA: Atoms contain tiny, negatively charged electrons. ᅞB: Atoms are always in motion. ᅞC: Atoms contain a tiny, positively charged nucleus. ᅞD: Atoms that combine do so in simple whole-number ratios.
Atoms contain tiny, negatively charged electrons.
What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide? ᅞA: Br2 + NaI --> NaBr2 + I ᅚB: Br2 + 2NaI --> 2NaBr + I2 ᅞC: Br + NaI2 --> NaBrI2 ᅞD: Br + NaI2 --> NaBr + I2
Br2 + 2NaI --> 2NaBr + I2
A 20.0-g sample of sucrose contains 8.4 g of carbon. What is the mass percentage of carbon in sucrose?
C: 42 %
Which of the following measurements is expressed to three significant figures? ᅞA: 0.007 m ᅞB: 7077 mg ᅚC: 7.30 x 10-3 km ᅞD: 0.070 mm
C: 7.30 x 10-3 km
Which model of the atom is thought to be true? ᅞA: Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom. ᅞB: The nucleus is made of protons, electrons, and neutrons. ᅚC: Electrons are distributed around the nucleus and occupy almost all the volume of the atom. ᅞD: The nucleus is made of electrons and protons.
C: Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
How do vapors and gases differ?
C: Generally, a gas is in the gaseous state at room temperature and a vapor is in either the solid state or liquid state at room temperature
What is the element with the lowest electronegativity value? ᅚA: cesium ᅞB: helium ᅞC: calcium ᅞD: fluorine
Cesium bigger atoms have lower electronegativity
Separating a solid from a liquid by evaporating the liquid is called ____.
D: distillation
Which sentence best describes a scientific theory?
It is well-tested and explains a wide range of observations
What characteristic must be true of a good hypothesis?
It must be testable by observation or experiment.
Which of the following elements has the smallest ionic radius? ᅚA: Li ᅞB: K ᅞC: O ᅞD: S
Li smaller if they form cations lithium get rid of electrons
What happens to matter during a chemical reaction A...Matter is neither destroyed or created. ᅞB: Some matter is destroyed. ᅞC: Some matter is created. ᅞD: Some matter is destroyed and some is created
Matter is neither destroyed or created.
Branch of chemistry regarding all carbon-containing matter
Organic Chemistry
What period 3 element having the following ionization energies (all in kJ/mol)? IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200
Phosphorus
What distinguishes a substance from a mixture?
The composition of substances cannot vary, while the composition of mixtures can
Who conducted experiments to determine the quantity of charge carried by an electron?
Thomson
Subtle differences in weight exist at different locations on Earth.
True
A resonance structure represents ᅞA: a difference in energy. ᅞB: electron pairs resonating back and forth between the extremes of the two structures. ᅞC: a difference in bond length, one shorter than the other. ᅚD: a hybrid of the extremes represented by the resonance forms.
a hybrid of the extremes represented by the resonance forms.
The closeness of a measurement to its true value is a measure of its
accuracy
Which type of radiation is the least penetrating?
alpha
Chemists who study the chemistry of living organisms work in the field of
biochemistry
The reaction 2Fe + 3Cl2 --> 2FeCl3 is an example of which type of reaction? ᅞA: combustion reaction ᅞB: single-replacement reaction ᅚC: combination reaction ᅞD: decomposition reaction
combination
A cathode ray consists of
electrons
4 Which of the following is a physical change? ᅞA: corrosion ᅞB: explosion ᅚC: evaporation ᅞD: rotting of food
evaporation
Which of the following is a heterogeneous mixture? ᅞA: hand lotion ᅞB: air ᅞC: stainless steel ᅚD: granite
granite
A controlled experiment is designed to test a(n)
hypothesis
A tentative or suggested answer to a question, formulated before experimentation, is called a(n)
hypothesis.
Which unit of measure is NOT used in the International System of Units
inches
The study of chemicals that, in general, do not contain carbon is traditionally called what type of chemistry?
inorganic
What is the SI unit of mass?
kilograms
Which state of matter has a definite volume and takes the shape of its container?
liquid only
Which of the following units is NOT an official SI unit?
liter
An example of an extensive property of matter is
mass.
A ________ can be used to help visualize microscopic structures and events.
model
An idea that describes how nature behaves but does not explain why nature behaves in the way it does is called a (n)
natural law
To what category of elements does an element belong if it is a poor conductor of electricity? ____ ᅞA: transition elements ᅞB: metalloids ᅚC: nonmetals ᅞD: metals
nonmetals
Which of the following is an example of an element?
oxygen
What are the horizontal rows in the periodic table called?
periods
What are quanta of light called? ᅞA: charms ᅞB: excitons ᅞC: muons ᅚD: photons
photons
The side-by-side overlap of p orbitals produces what kind of bond? ᅞA: alpha bond ᅞB: beta bond ᅚC: pi bond ᅞD: sigma bond
pi bond
The ability of a measurement to match the actual value of the quantity being measured is
precision
Which sub-atomic particles have approximately the same size and mass?
protons and neutrons
Research that is conducted for the sake of increasing fundamental knowledge is
pure research
Units of measurement are important to which type of data?
quantitative
What element has the electron configuration 1s2 2s2 2p6 3s2 3p2?
silicon
Which state of matter expands when heated and is easy to compress?
solid
When an iron nail is ground into powder, its mass ____.
stays the same
What is the basis of a metallic bond? ᅚA: the attraction of metal ions to mobile electrons ᅞB: the attraction between neutral metal atoms ᅞC: the neutralization of protons by electrons ᅞD: the attraction of oppositely charged ions
the attraction of metal ions to mobile electrons
Calculate the wavelength (in nm) of red light emitted by a neon sign with a frequency of 4.74 E14 Hz.
the speed of light ÷ frequency (3.00 × 108 m/s) = 633 nm
How many significant figures are in the measurement 0.003 4 kg?
two
A factor in an experiment that can change is a(n)
variable
The amount of space an object occupies is known as its
volume
What is the measurement of matter whose value depends on the force of gravity?
weight
A theory is a ____.
well-tested explanation for a broad set of observations
How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3 ᅚA: 1 ᅞB: 2 ᅞC: 3 ᅞD: 4 ᅞE: 0
ᅚA: 1
What are the coefficients that will balance the skeleton equation below? AlCl3 + NaOH --> Al(OH)3 + NaCl ᅚA: 1, 3, 1, 3 ᅞB: 3, 1, 3, 1 ᅞC: 1, 1, 1, 3 ᅞD: 1, 3, 3, 1
ᅚA: 1, 3, 1, 3
What is the wavelength of an electromagnetic wave that travels at 3 X 108 m/s and has a frequency of 60 MHz? (1 MHz = 1,000,000 Hz)
ᅚA: 300,000,000 m/s / 60,000,000 Hz covert MHZ to 60,000,000 HZ - - then speed ÷ frequency
How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain? ᅚA: 50 protons, 50 electrons, 75 neutrons ᅞB: 75 electrons, 50 protons, 50 neutrons ᅞC: 120 neutrons, 50 protons, 75 electrons ᅞD: 70 neutrons, 75 protons, 50 electrons
ᅚA: 50 protons, 50 electrons, 75 neutrons protons + Neutrons = mass number protons = electrons
What is the correct formula for barium chlorate? ᅚA: Ba(ClO3)2 ᅞB: Ba(ClO4)2 ᅞC: BaCl2
ᅚA: Ba(ClO3)2
Which of the following atoms has the greatest (most negative) electron affinity? ᅚA: CI. ᅞB: O. ᅞC: Be. ᅞD: Rb. ᅞE: I.
ᅚA: CI. more to the right is has the most negative electron affinity
Which of the following covalent bonds is the most polar? ᅚA: HಧF ᅞB: HಧC ᅞC: HಧH ᅞD: HಧN
ᅚA: HಧF
In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly? ᅚA: In, 49 protons, 49 electrons ᅞB: Zn, 30 protons, 60 electrons ᅞC: Cs, 55 protons, 132.9 electrons ᅞD: F, 19 protons, 19 electrons 1/1
ᅚA: In, 49 protons, 49 electrons
One of the products when aqueous Na2CO3 reacts with aqueous Sn(NO3)2 is ᅚA: NaNO3. ᅞB: NaSn. ᅞC: Sn(CO3)2. ᅞD: CNO3.
ᅚA: NaNO3.
Which of the following diatomic molecules is joined by a double covalent bond? ᅚA: O2 ᅞB: Cl2 ᅞC: N2 ᅞD: He2
ᅚA: O2
Which of the following compounds contains the lead(II) ion? ᅚA: PbO ᅞB: Pb2O ᅞC: PbCl4 ᅞD: Pb2S
ᅚA: PbO
Which of the following statements is true? ᅚA: Protons are positively charged and have a mass of 1 amu. ᅞB: Electrons are negatively charged and have a mass of 1 amu. ᅞC: The nucleus of an atom is positively charged and never has a mass of 1 amu. ᅞD: Neutrons are negatively charged and have a mass of 1 amu.
ᅚA: Protons are positively charged and have a mass of 1 amu.
What characteristic of metals makes them good electrical conductors? ᅚA: They have mobile valence electrons. ᅞB: They have mobile protons. ᅞC: They have mobile cations. ᅞD: Their crystal structures can be rearranged easily.
ᅚA: They have mobile valence electrons.
Most ionic compounds ᅚA: are crystalline solids at room temperature. ᅞB: have low melting points. ᅞC: conduct an electric current in the solid state. ᅞD: are composed of nonmetallic elements.
ᅚA: are crystalline solids at room temperature.
The equation H3PO4 + 3KOH --> K3PO4 + 3H2O is an example of which type of reaction? ᅚA: double-replacement reaction ᅞB: combination reaction ᅞC: decomposition reaction ᅞD: single-replacement reaction
ᅚA: double-replacement reaction
Emission of light from an atom occurs when an electron ᅚA: drops from a higher to a lower energy level. ᅞB: jumps from a lower to a higher energy level. ᅞC: moves within its atomic orbital. ᅞD: falls into the nucleus.
ᅚA: drops from a higher to a lower energy level.
Which of the following properties would you expect to find in a small, nonpolar molecule? ᅚA: gas at room temperature ᅞB: solid at room temperature ᅞC: very high melting point ᅞD: very high boiling point
ᅚA: gas at room temperature
Elements that are characterized by the filling of p orbitals are classified as ____. ᅚA: groups 3A through 8A ᅞB: transition metals ᅞC: inner transition metals ᅞD: groups 1A and 2A
ᅚA: groups 3A through 8A
What is the name of the compound whose formula is FeSO4?
ᅚA: iron(II) sulfate
Which of the following pairs of elements is most likely to form an ionic compound? ᅚA: magnesium and fluorine ᅞB: nitrogen and sulfur ᅞC: oxygen and chlorine ᅞD: sodium and aluminum
ᅚA: magnesium and fluorine
Which of the following quantum leaps would be associated with the greatest energy of emitted light? ᅚA: n = 5 to n = 1 ᅞB: n = 4 to n = 5 ᅞC: n = 2 to n = 5 ᅞD: n = 5 to n = 4
ᅚA: n = 5 to n = 1
If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals? ᅚA: one electron in each orbital ᅞB: two electrons in one orbital, one in another, none in the third ᅞC: three in one orbital, none in the other two ᅞD: Three electrons cannot fill three empty 2p atomic orbitals.
ᅚA: one electron in each orbital
Each period in the periodic table corresponds to a(n) ____. ᅚA: principal energy level ᅞB: energy sublevel ᅞC: orbital ᅞD: suborbital
ᅚA: principal energy level
What is shown by the structural formula of a molecule or polyatomic ion? ᅚA: the arrangement of bonded atoms ᅞB: the number of ionic bonds ᅞC: the number of metallic bonds ᅞD: the shapes of molecular orbitals
ᅚA: the arrangement of bonded atoms
The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ᅚA: the same. ᅞB: different from each other. ᅞC: the same as those of several other elements. ᅞD: the same as each other only in the ultraviolet range.
ᅚA: the same.
What is the charge on the cation in the ionic compound sodium sulfide? ᅞA: 0 ᅚB: 1+ ᅞC: 22+ ᅞD: 33+
ᅚB: 1+
Determine the electron configuration for phosphorus. ᅞA: 1s2 2s2 2p6 3p5 ᅚB: 1s2 2s2 2p6 3s2 3p3 ᅞC: 1s2 2s2 2p6 3s5 ᅞD: 1s2 2s2 2p6 3s1 3p4
ᅚB: 1s2 2s2 2p6 3s2 3p3
How many sigma and pi bonds are in the structural formula of carbon dioxide? ᅞA: 1 sigma 1 pi ᅚB: 2 sigma 2 pi ᅞC: 3 sigma 1 pi ᅞD: 1 sigma 3 pi
ᅚB: 2 sigma 2 pi
Which of the following isotopes has the same number of neutrons as phosphorus-31? ᅞA: 3215P ᅚB: 3216S ᅞC: 2914Si ᅞD: 2814Si
ᅚB: 32 16S
What is the formula for magnesium iodide? ᅞA: MgI ᅚB: MgI2 ᅞC: Mg2I ᅞD: Mg2I2 ᅞE: None of these are correct.
ᅚB: MgI2
What is the formula for sodium sulfate?
ᅚB: Na2SO4
10 How do the energy differences between the higher energy levels of an atom compare with the energy differences between the lower energy levels of the atom? ᅞA: They are greater in magnitude than those between lower energy levels. ᅚB: They are smaller in magnitude than those between lower energy levels. ᅞC: There is no significant difference in the magnitudes of these differences. ᅞD: No answer can be determined from the information given.
ᅚB: They are smaller in magnitude than those between lower energy levels.
Which of the following elements has the smallest atomic radius? ᅞA: sulfur ᅚB: chlorine ᅞC: selenium ᅞD: bromine
ᅚB: chlorine
Classify the following reaction: Li3PO4 ---> 3Li + P + 2O2 ᅞA: direct combination reaction ᅚB: decomposition reaction ᅞC: single-replacement reaction ᅞD: double-replacement reaction ᅞE: acid-base reaction
ᅚB: decomposition reaction
Which type of radiation is unaffected by magnetism? ᅞA: alpha ᅚB: gamma ᅞC: beta ᅞD: no type of radiation is affected by magnetism
ᅚB: gamma
What is the energy required to remove an electron from an atom in the gaseous state called? ᅞA: nuclear energy ᅚB: ionization energy ᅞC: shielding energy ᅞD: electronegative energy
ᅚB: ionization energy
All atoms of the same element have the same ____. ᅞA: number of neutrons ᅚB: number of protons ᅞC: mass numbers ᅞD: mass
ᅚB: number of protons
A net ionic equation ᅞA: shows the spectator ions. ᅚB: shows only those particles involved in the reaction. ᅞC: is not necessarily balanced with respect to mass or charge. ᅞD: shows dissolved ionic compounds as dissociated free ions.
ᅚB: shows only those particles involved in the reaction.
What shape does a boron trichloride molecule have?
ᅚB: trigonal planar
Which of the following measurements contains two significant figures? ᅞA: 0.004 00 L ᅞB: 0.004 04 L ᅚC: 0.000 44 L ᅞD: 0.004 40 L
ᅚC: 0.000 44 L
What happens to the bonds between atoms in a substance that undergoes a chemical reaction? ᅞA: All single covalent bonds become double covalent bonds. ᅞB: Some existing bonds will weaken while others strengthen. ᅚC: Existing bonds are broken and atoms are rearranged with the formation of new bonds. ᅞD: Bonds between atoms are unaffected during a chemical reaction.
ᅚC: Existing bonds are broken and atoms are rearranged with the formation of new bonds
The energy change from an added electron is called ᅞA: ionization energy. ᅞB: electronegativity. ᅚC: electron affinity. ᅞD: bond energy.
ᅚC: electron affinity.
20 In the Bohr model of the atom, an electron in an orbit has a fixed ____. ᅞA: position ᅞB: color ᅚC: energy ᅞD: size
ᅚC: energy
The principal quantum number indicates what property of an electron? ᅞA: position ᅞB: speed ᅚC: energy level ᅞD: electron cloud shape
ᅚC: energy level
Which of the following is a physical property? A: explosive ᅞB: combustible ᅚC: melting point ᅞD: ability to rust
ᅚC: melting point
A bond formed between a silicon atom and an oxygen atom is likely to be ____. ᅞA: ionic ᅞB: coordinate covalent ᅚC: polar covalent ᅞD: nonpolar covalent
ᅚC: polar covalent
Classify the following reaction: CS2 + 2 F2 ---> CF4 + 2S ᅞA: direct combination reaction ᅞB: decomposition reaction ᅚC: single-replacement reaction ᅞD: double-replacement reaction ᅞE: acid-base reaction
ᅚC: single-replacement reaction
Draw the Lewis structure for SO3. What is the hybridization on the S atom? ᅞA: sp ᅞB: sp3 ᅚC: sp2 ᅞD: sp3d ᅞE: sp3d2
ᅚC: sp2
Chemical equations must be balanced to satisfy ᅞA: the law of definite proportions. ᅞB: the law of multiple proportions. ᅚC: the law of conservation of mass. ᅞD: Avogadroಬs principle.
ᅚC: the law of conservation of mass.
When the following equation is balanced, what is the coefficient for HCl? Mg(s) + HCl(aq) --> MgCl2(aq) + H2(g) ᅞA: 6 ᅞB: 3 ᅞC: 1 ᅚD: 2
ᅚD: 2
When the equation for the complete combustion of one mole of C3H7OH is balanced, the coefficient for oxygen is ᅞA: 13/2 ᅞB: 11/2 ᅞC: 7/2 ᅚD: 9/2
ᅚD: 9/2
Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements? ᅞA: Henry Moseley ᅞB: Antoine Lavoisier ᅞC: John Dalton ᅚD: Dmitri Mendeleev
ᅚD: Dmitri Mendeleev
Who classified elements into triads? ᅞA: Mendeleev ᅞB: Moseley ᅞC: Newlands ᅚD: Dobereiner
ᅚD: Dobereiner
What is the correct formula for potassium sulfite? ᅞA: KHSO3 ᅞB: KSO4 ᅞC: K2HSO3 ᅚD: K2SO3
ᅚD: K2 SO3
Who predicted that all matter can behave as waves as well as particles? ᅞA: Albert Einstein ᅞB: Erwin Schrodinger ᅞC: Max Planck ᅚD: Louis de Broglie
ᅚD: Louis de Broglie
Use the activity series of metals to complete a balanced chemical equation for the following single replacement reaction. Ag(s) + KNO3(aq) -->
ᅚD: No reaction takes place because silver is less reactive than potassium.
Place the following elements in order of decreasing atomic radius. Xe Rb Ar ᅞA: Ar > Xe > Rb ᅞB: Xe > Rb > Ar ᅞC: Ar > Rb > Xe ᅚD: Rb > Xe > Ar ᅞE: Rb > Ar > Xe
ᅚD: Rb > Xe > Ar
If a combination reaction takes place between rubidium and bromine, the chemical formula for the product is
ᅚD: RbBr
Which of the following is a chemical change? ᅞA: breaking a pencil in half ᅞB: ice melting ᅞC: alcohol evaporating ᅚD: a banana rotting
ᅚD: a banana rotting
Which of the following is a chemical property? ᅞA: color ᅞB: hardness ᅞC: freezing point ᅚD: ability to react with oxygen
ᅚD: ability to react with oxygen
Electronegativity is the ability of an atom to ᅞA: release electrons. ᅞB: become an ion. ᅞC: conduct an electric current. ᅚD: attract electrons in a chemical bond.
ᅚD: attract electrons in a chemical bond.
According to the aufbau principle, ᅞA: an orbital may be occupied by only two electrons. ᅞB: electrons in the same orbital must have opposite spins. ᅞC: electrons enter orbitals of highest energy first. ᅚD: electrons enter orbitals of lowest energy first.
ᅚD: electrons enter orbitals of lowest energy first.
Which variable is directly proportional to frequency? ᅞA: wavelength ᅞB: velocity ᅞC: position ᅚD: energy
ᅚD: energy
Stable electron configurations are likely to contain ᅞA: high-energy electrons. ᅞB: unfilled s orbitals. ᅞC: fewer electrons than unstable configurations. ᅚD: filled energy sublevels
ᅚD: filled energy sublevels
Which of the following elements can form diatomic molecules held together by triple covalent bonds? ᅞA: carbon ᅞB: oxygen ᅞC: fluorine ᅚD: nitrogen
ᅚD: nitrogen
Under what conditions can potassium bromide conduct electricity? ᅞA: only when melted ᅞB: only when dissolved ᅞC: only when it is in crystal form ᅚD: only when melted or dissolved in water
ᅚD: only when melted or dissolved in water
Chemical reactions ᅞA: occur only in living organisms. ᅞB: create and destroy atoms. ᅞC: only occur outside living organisms. ᅚD: produce new substances.
ᅚD: produce new substances.
Draw a Lewis structure for the NH3 molecule. What is the hybrid orbital set used by the nitrogen atom for bonding? ᅞA: sp3d2 ᅞB: sp ᅞC: sp3d ᅚD: sp3 ᅞE: sp2
ᅚD: sp3
Which of the following is necessary to calculate the atomic mass of an element? ᅞA: the atomic mass of carbon-12 ᅞB: the atomic number of the element ᅞC: the relative masses of the elementಬs protons and neutrons ᅚD: the masses and relative abundance of each isotope of the element
ᅚD: the masses and relative abundance of each isotope of the element
Which color of visible light has the shortest wavelength? ᅞA: yellow ᅞB: green ᅞC: blue ᅚD: violet
ᅚD: violet
What would be the best name for Cr(OH)3? ᅞA: Mono Chromium Trioxide Trihydride ᅞB: Chromium Trioxide Trihydride ᅞC: Chromium Trihydroxide ᅞD: Chromium Hydroxide ᅚE: Chromium (III) Hydroxide
ᅚE: Chromium (III) Hydroxide
Of the metals in Group 1, which has the highest ionization energy? ᅞA: Cs. ᅞB: Rb. ᅞC: K. ᅞD: Na. ᅚE: Li.
ᅚE: Li. smallest has most ionization energy