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Chapter 2: The Chemical Context of Life
 
Chapter Quiz
 

Chapter Quiz


1 .       There are _____ naturally occurring elements. (Concept 2.1E-Book) [Hint]

 4
 25
 92
 108
 238
2 .       Which of the following is a trace element? (Concept 2.1E-Book) [Hint]

 hydrogen
 copper
 oxygen
 nitrogen
 carbon
3 .       Which one of the following is not one of the four most abundant elements found in living systems? (Concept 2.1E-Book) [Hint]

 hydrogen
 nitrogen
 carbon
 zinc
 oxygen
4 .       Which one of the following has negligible mass? (Concept 2.2E-Book) [Hint]

 proton
 neutron
 electron
 atom
 element
5 .       Which one of the following subatomic particles has appreciable mass and lacks a charge? (Concept 2.2E-Book) [Hint]

 proton
 neutron
 electron
 element
 molecule
6 .       The number of protons in an uncharged atom _____. (Concept 2.2E-Book) [Hint]

 equals the number of electrons
 equals the number of neutrons
 varies with the different isotopes
 equals the number of electrons in the outer orbital of the atom
 determines its mass number
7 .       Consider a hypothetical atom with an atomic number of 4 and a net electronic charge of +1. How many neutrons does this atom have? (Concept 2.2E-Book) [Hint]

 1
 3
 4
 The answer cannot be determined from the information provided.
 none of the above
8 .       An element has 8 protons, 9 neutrons, and 8 electrons. Its atomic number and atomic mass, respectively, are _____. (Concept 2.2E-Book) [Hint]

 8 and 16
 8 and 17
 9 and 16
 9 and 17
 16 and 8
9 .       Two atoms of the same element must have the same number of _____. (Concept 2.2E-Book) [Hint]

 neutrons
 protons
 electrons
 neutrons plus protons
 protons plus electrons
10 .       An uncharged atom of nitrogen (atomic number = 7) has _____. (Concept 2.2E-Book) [Hint]

 7 neutrons
 7 protons and 7 neutrons
 7 neutrons and 7 electrons
 7 protons and 7 electrons
 7 valence electrons
11 .       Isotopes of an element will always differ in _____. (Concept 2.2E-Book) [Hint]

 atomic number
 atomic mass
 number of electrons
 number of protons
 none of the above
12 .       A particular carbon isotope has an atomic number of 6 and an atomic mass of 14. The respective number of neutrons, protons, and electrons that this carbon isotope has is _____. (Concept 2.2E-Book) [Hint]

 6, 8, and 6
 6, 6, and 8
 8, 6, and 6
 8, 6, and 8
 8, 6, and 4
13 .       Phosphorus-32 (radioactive) has _____ than phosphorus-35 (normal). (Concept 2.2E-Book) [Hint]

 3 more neutrons
 3 more protons
 3 fewer neutrons
 3 fewer protons
 three more atoms
14 .       The most common form of calcium has 20 protons, 20 neutrons, and 20 electrons. Which of the following elements would be an isotope of calcium? (Concept 2.2E-Book) [Hint]

 an atom with 21 protons, 20 neutrons, and 21 electrons
 an atom with 20 protons, 20 neutrons, and 18 electrons
 an atom with 20 protons, 21 neutrons, and 20 electrons
 an atom with 21 protons, 21 neutrons, and 21 electrons
 all of the above
15 .       Which of the following is not a characteristic that makes radioactive tracers useful in medical diagnoses? (Concept 2.2E-Book) [Hint]

 They are incorporated into reactions in living material.
 They are easily detectable in minute amounts.
 They may damage or destroy molecules.
 Living cells cannot distinguish them from nonradioactive isotopes.
 They can be used with PET scanners.
16 .       Potassium (atomic number 19, mass number 40) and sodium (atomic number 11, mass number 23) have similar chemical properties and reactive behavior. This is because uncharged atoms of potassium and sodium _____. (Concept 2.2E-Book) [Hint]

 have different atomic numbers but the same number of electrons
 have different atomic numbers and different numbers of electrons in their outermost electron shells
 have the same atomic number and each has 1 electron in its outermost electron shell
 have different mass numbers and each has 1 electron in its outermost electron shell
 have different atomic numbers, different mass numbers, and different numbers of electrons in their outermost electron shells
17 .       Atomic chlorine has an atomic number of 17. It has _____ electrons in its third shell. (Concept 2.2E-Book) [Hint]

 2
 7
 8
 10
 17
18 .       The chemical characteristics or reactivity of an element depend mostly on the _____. (Concept 2.2E-Book) [Hint]

 number of electrons in its outermost shell
 number of electron shells present in the atoms
 mean energy level of its electrons
 degree to which it has more or fewer electrons than protons
 number of protons plus the number of neutrons
19 .       Some groups of elements react chemically in similar ways. For example, the chemistry of sodium and the chemistry of lithium are similar. The chemistry of chlorine and the chemistry of iodine are also similar. These similarities in chemistry result when different elements have similar _____. (Concept 2.2E-Book) [Hint]

 atomic size
 numbers of outer-shell electrons
 total numbers of electrons
 energy quanta per electron
 atomic number
20 .       How many electrons would be present in the valence shell of a sulfur atom (atomic number 16, mass number 32)? (Concept 2.2E-Book) [Hint]

 1 electron
 2 electrons
 4 electrons
 6 electrons
 8 electrons
21 .       For most atoms, a stable configuration of electrons is attained when the atom _____. (Concept 2.2E-Book) [Hint]

 has as many protons as neutrons
 has moved all its electrons to its outermost shell
 achieves a zero net charge
 has 8 electrons in its outermost shell
 none of the above
22 .       An atom that normally has _____ in its outer shell would not tend to form chemical bonds with other atoms. (Concept 2.2E-Book) [Hint]

 1 electron
 3 electrons
 4 electrons
 6 electrons
 8 electrons
23 .       A polar covalent bond is a bond that _____. (Concept 2.3E-Book) [Hint]

 is found only in H2O
 is found only in molecules containing oxygen
 shares electrons equally between atoms
 ionizes
 has shared electrons pulled closer to the more electronegative atom
24 .       A covalent bond is likely to be polar if _____. (Concept 2.3E-Book) [Hint]

 the two atoms sharing electrons are equally electronegative
 one of the atoms sharing electrons is much more electronegative
 it is between two atoms that are both very strong electron acceptors
 the two atoms sharing electrons are of the same element
 it is between two atoms that are both very strong electron donors
25 .       When the proton number and electron number are unequal, the atom or molecule _____. (Concept 2.3E-Book) [Hint]

 forms a covalent bond with another atom
 is an ion
 becomes part of a molecule
 gains or loses a proton
 gains or loses a neutron
26 .       A sodium atom has a mass number of 23. Its atomic number is 11. How many electrons does it have if it is not an ion? (Concept 2.3E-Book) [Hint]

 11
 12
 22
 23
 34
27 .       Copper has an atomic number of 29 and a mass number of 64. What would result if an uncharged copper atom lost two electrons? (Concept 2.3E-Book) [Hint]

 The atom would have a double negative charge and be an ion.
 The atomic number of the atom would remain 29, the mass number would be reduced to 62, and the atom would be an anion.
 The atomic number would remain 29, the mass number would increase to 66, and the atom would be a cation with a -2 charge.
 The atomic number would be reduced to 27, the mass number would remain 64, and the atom would be an anion with a +2 charge.
 The atomic number would remain 29, the mass number would remain 64, and the atom would be a cation with a +2 charge.
28 .       The compound CaSO4 ionizes into a calcium ion and a sulfate ion (SO4). Calcium has 2 electrons in its outer shell. Upon ionization, what would you expect the charge on the sulfate ion to be? (Concept 2.3E-Book) [Hint]

 -4
 +2
 +1
 -1
 -2
29 .       Ionic bonds form as a result of _____. (Concept 2.3E-Book) [Hint]

 attraction between atoms that have opposite charges
 attraction between hydrogen and other atoms that share electrons unequally
 sharing of electron pairs between atoms
 unequal sharing of electrons between atoms
 the asymmetric distribution of electrons in constant motion
30 .       A hydrogen bond _____. (Concept 2.3E-Book) [Hint]

 is one in which two hydrogen atoms bond to each other
 is one in which hydrogen is strongly attracted to a positively charged atom
 is a function of hydrophobic interactions
 is a weak chemical bond
 is a strong chemical bond
31 .       Which is not involved in, or is not relevant to, hydrogen bonding? (Concept 2.3E-Book) [Hint]

 attraction of electrons by one atom more than another
 partial electrical charges
 attraction between unlike partial charges
 loss of electrons
 polar molecules
32 .       Hydrogen bonds occur when _____. (Concept 2.3E-Book) [Hint]

 a molecule with partial charges contacts a molecule without partial charges
 a molecule with a low molecular weight is bonded to a molecule with a high molecular weight
 two atoms achieve stable electron configurations by sharing electrons with each other
 partial opposite charges on molecules come close enough to attract each other
 none of the above
33 .       Which of the following molecules has the shape of a completed tetrahedron? (Concept 2.3E-Book) [Hint]

 water (H2O)
 hydrogen gas (H2)
 oxygen gas (O2)
 methane (CH4)
 glucose (C6H12O6)
34 .       Which of the following statements is not true about chemical reactions? (Concept 2.4E-Book) [Hint]

 They represent the way matter is created and destroyed.
 They convert reactants to products.
 They always have the same number of a given atom on each side of the equation arrow.
 They involve the making and breaking of chemical bonds.
 They can involve organic as well as inorganic molecules.
35 .       Which one of the following does the equation of a chemical reaction not tell us? (Concept 2.4E-Book) [Hint]

 the number of atoms or molecules involved
 the kinds of atoms or molecules involved
 the direction in which the reaction occurs
 the speed of the reaction
 A chemical equation describes all the above features.
36 .       Which of the following statements describes a reversible reaction that has reached chemical equilibrium? (Concept 2.4E-Book) [Hint]

 The rate of the reverse reaction exceeds the rate of the forward reaction.
 The rate of the reverse reaction equals the rate of the forward reaction.
 The rate of the forward reaction exceeds the rate of the reverse reaction.
 The forward and the reverse reactions have stopped.
 The concentration of the reactants is equal to the concentration of the products.





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