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Physic
Q:
Which of the following is an ion?
A) 2 H2
B) Br2
C) HCl
D) Au + 3 Br2
E) none of the above
Q:
If a neutral atom loses one electron, what is the electrical charge of the atom?
A) -1
B) +1
C) -2
D) +2
E) neutral
Q:
If a neutral atom gains two electrons, what is the electrical charge of the atom?
A) -1
B) +1
C) -2
D) +2
E) neutral
Q:
What needs to be done to convert a neutral nitrogen atom into an N-3 species?
A) add three electrons
B) remove three electrons
C) remove three protons
D) add three protons
E) add three nitrogens
Q:
Which of the following is a positive ion?
A) Na+1
B) Ca+2
C) Mg+2
D) Al+3
E) all of the above
Q:
Which of the following is a negative ion?
A) Na+1
B) Na
C) O-2
D) O
E) all of the above
Q:
Which of the following would be a negative ion with a single charge?
A) an atom with 11 protons and 12 electrons
B) an atom with 11 protons and 11 electrons
C) an atom with 12 protons and 11 electrons
D) an atom with 10 protons and 12 electrons
E) none of the above
Q:
Which of the following would be an ion with a double positive charge?
A) an Mg atom that gains two electrons
B) an Mg atom that gains one electron
C) an Mg atom that loses two electrons
D) an Mg atom that loses one electron
E) none of the above
Q:
Which of the following elements will most likely form an ion with a +1 charge?
A) Na
B) Mg
C) Al
D) Si
E) Cl
Q:
Which of the following elements will most likely form an ion with a +2 charge?
A) Na
B) Mg
C) Ne
D) Si
E) Cl
Q:
Which of the following elements will most likely form an ion with a -2 charge?
A) Na
B) S
C) Ne
D) Mg
E) Cl
Q:
Which of the following elements will most likely form an ion with a -1 charge?
A) Na
B) S
C) Ne
D) Mg
E) Cl
Q:
Which of the following elements will most likely not form an ion at all?
A) Na
B) O
C) Ar
D) Mg
E) Br
Q:
What is the name for the following polyatomic ion?
PO4-3
A) phosphate
B) phosphorus oxide
C) phosphinate
D) trioxo phosphoride
E) potassium
Q:
What is the name for the following polyatomic ion?
CH3CO2-1
A) acetate
B) monocarboxylate
C) carboxylic
D) acidic
E) acetic
Q:
If carbonic acid (H2CO3) were to undergo ionization, what would one of the products be?
A) H-
B) CO2
C) H2O
D) CO3-1
E) CO3-2
Q:
How is it possible for a neutral molecule, such as water, to form an ion?
A) It can combine with a hydrogen ion to form a positively charged species.
B) It can combine with a chloride ion to form a negatively charged species.
C) It can fragment into protons and electrons.
D) It can absorb electrons and become negatively charged.
E) It can absorb electrons and become positively charged.
Q:
An atom loses an electron to another atom. Is this an example of a physical or chemical change?
A) physical change involving the formation of negative ions
B) chemical change involving the formation of neutral atoms
C) physical change involving the formation of positive ions
D) chemical change involving the formation of ions
Q:
Why is it so easy for a magnesium atom to lose two electrons?
A) The nuclear charge of the magnesium atoms is relatively weak.
B) These two electrons are found relatively far from the nucleus.
C) These two electrons are well shielded from the nuclear charge.
D) There are lots of electron-electron repulsions that go on within the valence shell.
Q:
How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form?
A) There is no defined relationship between the number of unpaired valence electrons and number of bonds that the atom can form.
B) The number of unpaired valence electrons in an atom is one-half the number of bonds that the atom can form.
C) The number of unpaired valence electrons in an atom is twice the number of bonds that the atom can form.
D) The number of unpaired valence electrons in an atom is the same as the number of bonds that the atom can form.
Q:
How many more electrons can fit within the valence shell of a hydrogen atom?
A) 1
B) 2
C) 7
D) 0
Q:
How do the electron-dot structures of elements in the same group in the periodic table compare with one another?
A) The structures differ by exactly two electrons between vertically consecutive elements.
B) The number of valence shell electrons increases by one for each element from the top to the bottom of the group.
C) Elements of the same group have the same number of valence electrons.
D) The number of electrons in the electron-dot-structure will equal the group number for each element of the group.
Q:
What is one role of unpaired valance electrons?
A) They take part in the formation of different types of bonds.
B) They keep the paired electrons separated to minimize interaction.
C) They are the nonbonding electrons.
D) They provide the number of Lewis dots.
E) They tell us which Lewis dot structure is correct.
Q:
Which of the following elements has two valence electrons?
A) Na
B) Mg
C) H
D) Ne
E) Li
Q:
Which of the following elements has six valence electrons?
A) Be
B) B
C) C
D) N
E) O
Q:
How many valence electrons does bromine (Br, atomic no. = 35) have?
A) 1
B) 7
C) 21
D) 28
E) 35
Q:
How many valence electrons does gallium (Ga, atomic no. = 31) have?
A) 1
B) 6
C) 3
D) 31
E) 70
Q:
How many valence electrons does boron (B, atomic no. = 5) have?
A) 1
B) 2
C) 3
D) 4
E) 5
Q:
Which of the following has the greatest number of nonbonding pairs of electrons?
A) C
B) H
C) He
D) F
E) S
Q:
Which of the following is the correct electron dot structure for carbon (atomic no. = 6)? A) a
B) b
C) c
D) d
E) e
Q:
Which of the following is the correct electron dot structure for chlorine (atomic no. = 17)? A) a
B) b
C) c
D) d
E) e
Q:
Many of the macroscopic properties of a compound depend on
A) how the atoms of the molecules are held together.
B) the mass of the constituent atoms.
C) the number of nucleons present in the sample.
D) the size of the sample.
E) how the atoms absorb light and the shape of the orbitals.
Q:
The concept of a chemical bond is
A) how two or more atoms are held together.
B) the sharing of nucleons.
C) how two or more electrons reside in an orbital.
D) how much energy it takes to remove an electron from a set of atoms.
E) none of the above
Q:
Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds?
A) Ionic bonds are so much stronger than the molecular attractions between covalently bonded compounds.
B) Covalent bonds are not as strong as ionic bonds.
C) As a solid, salts have a very organized crystalline structure which takes a lot of energy to break apart.
D) Most covalent compounds have at least one weak bond in their structure that is easily broken when heat is added.
Q:
Two chemical structures are shown, one of a typical gasoline molecule and the other of a typical motor oil molecule. Which is which? Base your reasoning not on memorization but rather upon what you know about molecular interactions and the various physical properties of gasoline and motor oil.
A) Structure A represents the gas molecule because there are more bonds to gain energy from, giving it a higher energy content than oil.
B) Structure A represents motor oil, illustrating a molecule with greater induced dipole-induced dipole molecular interactions thus, the molecules are strongly attracted to one another.
C) Structure B represents the oil molecule. Because oil molecules are smaller, they can compact closer together, giving the appearance of a thicker solution than gasoline.
D) Structure B represents crude oil which is processed to generate longer molecules of gasoline to prevent toxic vapors from harming consumers.
Q:
The boiling point of 1,4-butanediol is 230C. Would you expect this compound to be soluble or insoluble in room-temperature water? A) Since there are no polar areas on this molecule, it is insoluble in water at room temperature.
B) A high boiling point means that the substance interacts with itself quite strongly. Therefore this molecule is not soluble in water.
C) Since there are polar areas on this molecule, it is insoluble in water at room temperature.
D) Water would be attracted to both ends of 1,4 butanediol, and it is infinitely soluble in water.
Q:
Consider the boiling points of the following compounds and their solubilities in room-temperature water. Why does the solubilities in water go down as the boiling points of these alcohols go up. A) Larger molecules are less attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions.
B) As the boiling increases, it is more difficult to keep the alcohol from evaporating out of solution.
C) As the boiling point increases, the size of the alcohol molecules decreases.
D) Larger molecules are more attracted to one another by induced dipole-induced dipole as well as by dipole-dipole and dipole-induced dipole attractions.
Q:
Why is the surface area of a gecko's foot so extensive?
A) A gecko, like all amphibians, needs extensive surface area under foot for stability on land as well as mobility in water.
B) A gecko's foot acts like a large dipole and thus allows for ion-dipole interaction in water.
C) The greater the surface area the greater the number of induced dipole-induced dipole forces of attraction that can occur between the gecko's foot and the surface.
D) The extensive surface area, once charged by the gecko's body, allows for the dipole-dipole attraction of every contact surface.
Q:
List the following compounds in order of increasing boiling point: , ,, .
A) , , , B) , , , C) , , , D) , , ,
Q:
How are oxygen molecules attracted to water molecules?
A) The attraction between oxygen and water molecules is a classic example of dipole-dipole interaction.
B) The hydrogen bonding in water causes the attraction of the oxygen atoms in the molecule to water.
C) As a water molecule is brought close to an oxygen molecule an induced dipole results in the molecule causing the attraction.
D) The attraction of oxygen and water molecules for one another is part of the common atom effect. Since both molecules contain oxygen, there is a built-in attraction.
Q:
Dipole-induced dipole forces of attraction exist between water and gasoline, and yet these two substances do not mix because water has such a strong attraction for itself. Which of the following compounds might best help to make these two substances mix into a single liquid phase? A) the molecule on the far left because the O-H bond is polar and the carbon and hydrogen bonds are nonpolar
B) the molecule in the middle because when the salts mix into the water, it will help separate the water and decrease the attraction for itself
C) The molecule on the right will form attractions with the polar ends of the water, allowing the gasoline a chance to mix with the water.
D) All of these molecules would be equally effective at increasing the mixing of gasoline and water.
Q:
Plastic wrap is made of nonpolar molecules and is able to stick well to polar surfaces, such as glass, by way of dipole/induced dipole molecular attractions. How is it that plastic wrap also sticks to itself so well?
A) by way of dipole-dipole molecular attractions
B) by way of dipole-induced dipole molecular attractions
C) Ions are formed as the plastic rubs against itself.
D) by way of induced dipole-induced dipole molecular attractions
Q:
Chlorine, , is a gas at room temperature, but bromine, , is a liquid. Explain.
A) Chlorine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable.
B) Bromine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable.
C) The smaller chlorine molecules are able to pack together in a tighter physical orientation.
D) The bromine ions are held together by ionic bonds.
Q:
Why are ion-dipole attractions stronger than dipole-dipole attractions?
A) The chemical bond in an ion-dipole molecule is similar also a covalent bond.
B) The magnitude of the electric charge associated with an ion is much greater.
C) Dipole areas are subject to changing from positive to negative regions on the molecule.
D) Like charge (dipole) does not attract like charge (another dipole).
Q:
Why is calcium fluoride, Ca, a high melting point crystalline solid while stannic chloride, , is a volatile liquid?
A) There is no theory to predict the physical property of melting point. Melting point temperatures are empirically determined.
B) Actually, we would predict these results to be the opposite. Since each metal is combined with a group 17 halogen, the heavier metal (tin) combination should have the higher melting point.
C) Ca is a small, linear, non-polar molecule, while is a huge tetrahedral structure. Therefore the bonds in calcium fluoride tend to give it a higher melting point temperature.
D) Ionic compounds formed by elements on opposite sides of the periodic table, like , tend to have higher melting points than more covalently bonded structures, like .
Q:
The charges with sodium chloride are all balanced-for every positive sodium ion there is a corresponding negative chloride ion. Since its charges are balanced, how can sodium chloride be attracted to water, and vice versa?
A) Dispersion forces come into play as the sodium chloride and water come into close proximity.
B) Hydrogen bonding in water allows the sodium chloride molecule to be attracted to the water molecule.
C) As a water molecule gets close to the sodium chloride it can distinguish the various ions and it is thus attracted to an individual ion by ion-dipole forces.
D) This is not a matter of attraction. Sodium chloride dissolves in water because water provides a medium in which the individual sodium and chloride ions can disperse.
Q:
Which of the following intermolecular forces best describes why molecules like CF3CF3 are soluble in liquid CO2?
A) dipole-dipole
B) induced dipole-induced dipole
C) dipole-induced dipole
D) ion-dipole
E) hydrogen bonding
Q:
Which of the following intermolecular forces best describes why molecules like sucrose (which has many OH groups) are very water soluble?
A) dipole-dipole
B) induced dipole-induced dipole
C) dipole-induced dipole
D) ion-dipole
E) hydrogen bonding
Q:
Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18) have only limited solubility in water?
A) dipole-dipole
B) induced dipole-induced dipole
C) dipole-induced dipole
D) ion-dipole
E) Both A and B
Q:
Which of the following would have the smallest number of induced dipole-induced dipole interactions?
A) C6H14
B) C8H18
C) C10H22
D) C12H26
E) not enough information given
Q:
Which of the following would have the highest boiling point?
A) C6H14
B) C8H18
C) C10H22
D) C12H26
E) not enough information given
Q:
Which of the following would have the lowest melting point?
A) CCl4
B) CBr4
C) CF4
D) CI4
E) not enough information given
Q:
Which of the following would have the highest boiling point?
A) Cl2
B) Br2
C) F2
D) I2
E) not enough information given
Q:
Which of the following is most likely to have the weakest induced dipole-induced dipole interaction?
A) Cl2
B) Br2
C) F2
D) I2
E) All of the above have the same interactions.
Q:
What is the main difference between a dipole-dipole interaction and a dipole-induced dipole interaction?
A) Both are similar, but one involves a temporary dipole created by a permanent dipole.
B) Dipole-dipole interactions are weaker because the dipoles are permanent.
C) Dipole-induced dipole interactions are stronger because the induced dipoles can be formed at any time.
D) Both are identical.
E) none of the above
Q:
In which of the following molecules will water induce a temporary dipole?
A) CO2
B) O2
C) N2
D) all of the above
E) none of the above
Q:
Given the following diagram, describe what happens electronically between these two molecules. A) Oxygen A becomes slightly positively charged due to the protons on the water molecule.
B) Oxygen B becomes slightly positively charged due to the protons on the water molecule.
C) Oxygen A becomes slightly negatively charged due to the oxygen molecule.
D) Hydrogens on oxygen W becomes slightly positively charged due to the oxygen molecule.
E) none of the above
Q:
Given the following diagram, describe what happens electronically between these two molecules. A) Oxygen B becomes slightly positively charged due to the electrons on the water molecule.
B) Oxygen A becomes slightly positively charged due to the electrons on the water molecule.
C) Oxygen W becomes slightly negatively charged due to the oxygen molecule.
D) Oxygen W becomes slightly positively charged due to the oxygen molecule.
E) none of the above
Q:
Which of the following is the main form of intermolecular attractions among water molecules?
A) hydrogen bonding
B) induced dipole-induced dipole
C) covalent bonding
D) ion-dipole
E) polar-induced polar
Q:
Which of the following molecules is most likely to show a dipole-dipole interaction?
A) H2S
B) CO2
C) CH4
D) H-CC-H
E) none of the above
Q:
Which of the following molecules is most likely to show a dipole-dipole interaction?
A) CH3OH
B) CH3SH
C) CH4
D) H-CC-H
E) A and B
Q:
Which of the following molecules is most likely to show the strongest hydrogen bonding?
A) CH3OH
B) CH3SH
C) CH4
D) H-CC-H
E) A, B and C
Q:
What is a hydrogen bond?
A) a special type of dipole-dipole attraction involving hydrogen bound to a highly electronegative atom
B) a special type of dipole-dipole attraction involving hydrogen bound to any other atom
C) a special type of dipole-dipole attraction involving hydrogen bound to another hydrogen atom
D) a special type of attraction involving any molecules that contain hydrogens
E) none of the above
Q:
Which of the following describes an aqueous solution?
A) a mixture of some compound dissolved in water
B) a mixture of polar molecules dissolved in a nonpolar solvent
C) a mixture of water dispersed in an ionic compound
D) a mixture of nonpolar molecules dissolved in a polar solvent
E) none of the above
Q:
What is the difference between a dipole-dipole interaction and an ion-dipole interaction?
A) one involves dipole attraction between neutral molecules while the other involves dipole interactions with ions
B) one involves hydrogen bonding while the other does not
C) one involves salts and water while the other doesn't involve water
D) one involves ionic molecules interacting with other ionic molecules while the other deals with polar molecules
E) none of the above
Q:
If an ionic bond is stronger than a dipole-dipole interaction, how can water dissolve an ionic compound?
A) The ion-dipole interactions of a bunch of water molecules gang up on the strong ionic bond and pull it into the solution.
B) The ionic bond is weakened by the ion-dipole interactions and ionic repulsion ejects the ions from the crystal.
C) The ion-dipole interaction causes the ions to heat up and vibrate free of the crystal.
D) The ions never overcome their interatomic attraction and therefore are not soluble.
E) none of the above
Q:
What is happening at the molecular level when a polar molecule like water interacts with a typical sodium ion?
A) The water molecule aligns such that the oxygen interacts with the sodium.
B) The water molecule aligns such that the hydrogens interact with the sodium.
C) The polarity of the water molecule is altered making the oxygen more positively charged.
D) The polarity of the water molecule is altered making the hydrogens more negatively charged.
E) none of the above
Q:
The separation of charges within a polar molecule is called a(n)
A) dipole.
B) dipole-dipole.
C) ionic bond.
D) strong attraction.
E) polar bond.
Q:
Which of the following molecules would you expect to be the most strongly attracted to a Cl- ion?
A) H-F
B) H3C-CH3
C) Cl-Cl
D) F-F
E) CCl4
Q:
Which of the following molecules would you expect to be the least attracted to a Na+ ion?
A) H-F
B) H3C-CH3
C) Cl2CH2
D) F-
E) HO-
Q:
Which of the following is the strongest?
A) a chemical bond
B) an ion-dipole attraction
C) a dipole-dipole attraction
D) a dipole-induced dipole attraction
E) an induced dipole-induced dipole attraction
Q:
Which of the following is the weakest?
A) a chemical bond
B) an ion-dipole attraction
C) a dipole-dipole attraction
D) a dipole-induced dipole attraction
E) an induced dipole-induced dipole attraction
Q:
Ammonia, N, is more polar than is borane, B because it
A) has a lone pair of electrons.
B) is less symmetrical than borane.
C) its hydrogens are not exactly opposite one another.
D) all of the above
Q:
A substance consisting of which molecule shown below should have a higher boiling point? A) The molecule on the left, CO, because it has a fewer number of atoms.
B) The molecule on the right, Cl, because it has a greater number of atoms.
C) The molecule on the left, CO, because it is less symmetrical.
D) The molecule on the right, Cl, because of electronegativity considerations.
Q:
An individual carbon-oxygen bond is polar. Yet carbon dioxide, C, which has two carbon-oxygen bonds, is nonpolar because
A) the molecule has an even number of electrons.
B) it has a greater symmetry.
C) the electron-pulls of the two oxygen atoms are equal and opposite.
D) Two of the above are reasonable.
Q:
Water, O, and methane, C, have about the same mass and differ by only one type of atom. Why is the boiling point of water so much higher than that of methane?
A) The water molecule is less symmetrical than is the methane molecule.
B) The oxygen of a water molecule has two lone pairs of electrons.
C) The electronegativity difference between oxygen and hydrogen is greater than the electronegativity difference between carbon and hydrogen.
D) all of the above
Q:
List the following bonds in order of increasing polarity.
A) N-O < N-N < N-F < H-F
B) N-N < N-O < N-F < H-F
C) H-F < N-F < N-O < N-N
D) N-N < N-O < H-F < N-F
Q:
Which of the following molecules is the most polar?
A) HCl
B) BrF
C) CO
D)
Q:
Which molecule is most polar?
A) S=C=S
B) O=C=O
C) O=C=S
D) These all have the same polarity.
Q:
Which of the following molecules should have the same molecular shape and approximate bond angles as ammonia, ?
A) B) C) D) E)