Chemistry 160 – Exam 4 – Flashcards
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The effective nuclear charge for an atom is less than the actual nuclear charge due to
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shielding
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Which of the following is a covalent compound?
a. Na2O
b. CaCl2
c. Cl2O
d. MgBr2
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Cl2O
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Identify the element of Period 2 that has the following successive ionization energies, in kJ/mol
1E1, 1314
1E2, 3389
1E3, 5298
1E4, 7471
1E5, 10992
1E6, 13329
1E7, 71345
1E8, 84087
a. Li
b. B
c. O
d. Ne
e. none of these is correct
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c. O
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Select the element with the greatest metallic character
a. Li
b. Ca
c. Al
d. Pb
e. Cs
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e. Cs
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Which of the following atoms will be diamagnetic?
a. Cr
b. Ru
c. Fe
d. Pt
e. Cd
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e. Cd - [Kr]5s2(4)d10
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Which of the following contains ionic bonding?
a. CO
b. SrF2
c. Al
d. OCl2
e. HCl
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c. SrF2
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In which of these substances are the atoms held together by polar covalent bonding?
a. SrCl2
b. CsCl
c. ClF
d. CaF2
e. S8
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c. ClF
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Which of the following elements has the largest atomic size?
a. Rn
b. Ca
c. Po
d. Ba
e. S
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d. Ba
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Which of the following elements is the most electronegative?
a. O
b. Li
c. F
d. I
e. Cl
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c. F (up and right)
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Which of the following compounds will have the highest lattice energy?
a. RbBr
b. LiF
c. KCl
d. LiCl
e. RbCl
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b. LiF
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Electronegativity is a measure of:
a) the energy needed to remove an electron from an atom
b) the energy released when an electron is added to an atom
c) the magnitude of the negative charge on an electron
d) the attraction by an atom for electrons in a chemical bond
e) the magnitude of the negative charge on a molecule
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d) the attraction by an atom for electrons in a chemical bond
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Which of the following elements will form a cation with a 2+ charge?
a) Si
b) Sr
c) Ga
d) Cs
e) S
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b) Sr
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Which of the following atoms/ions will have the smallest radius?
a) K+
b) K
c) Ca2+
d) Ca
e) Rb+
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a) K+
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Ionization Energy
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energy required to remove an electron
*greatest at top right
*lowest at bottom left
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Electron Affinity
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energy is required when a gaseous atom adds an e-
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Electronegativity
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Ability of atom to attract electrons away from other atoms in a compound
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Most electronegative element
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F
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Least electronegative element
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Cs
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Metallic Behavior
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Bottom left is most metallic
Top right is least metallic
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Ionic bonds
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transfer of e- between metal and nonmetal
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Covalent Bond
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sharing of e- between two or more nonmetals
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Metallic bond
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metals with metals
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Born Haber Cycle
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Allows for calculation of lattice energy - process of forming the compound from atoms in standard states
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lattice energy
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energy which holds ions together
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Lattice Energy
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k((Q+ x Q-)/(d))
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How can we make lattice energy larger?
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1. decrease distance b/w ions (smaller ions)
2. greater charge on ions
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Endothermic reaction
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e- is on the right side of the arrow
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Exothermic reaction
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e- is on the left side of the arrow & (g) + (g) = s
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Cations (+) are _________ than parent atoms. Electrons are ________ from the outer level.
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smaller, removed
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Anions (-) are _________ than parent atoms. Electrons are ________ from the outer level.
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larger, added
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Magnetic properties: paramagnetism
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Attracted to an external field (Not all 5 bond spots are full)
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Magnetic properties: Dimagnetic
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not attracted to the field (All 5 bond spots are full)
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Metal oxides act like a
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base
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Nonmetal oxides act like aN
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acid
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4 Exceptions to electron configuration
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Cr, Mo, Cu, Ag
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Oxidation number =
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# of valence electrons - (# shared e- + # of unshared e-)
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Determining Formal Charge
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# Valence - # Lone e - # of bonds
