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25 Cards in this Set
- Front
- Back
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What is the term for an atom (or group of atoms) that bears a charge as the result of gaining or losing valence electrons?
a. anion b. cation c. ion d. polyatomic ion e. none of the above |
c. ion
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What is the term for the electrons that occupy the outermost s and p sublevels of an atom?
a. core electrons b. kernel electrons c. sublevel electrons d. valence electrons e. none of the above |
d. valence electrons
These are those electrons that will more easily adhere to another element. |
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Why were noble gases absent from Mendeleev’s original periodic table of 1871?
a. The noble gases are unstable. b. The noble gases are radioactive. c. The noble gases had not been discovered. d. The noble gases occur only in compounds. e. none of the above |
c. The noble gases had not been discovered.
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Following the X-ray emission studies of Harry Moseley in 1913, the order of the elements in the periodic table was based on which of the following?
a. increasing atomic number b. increasing mass number c. increasing atomic mass d. increasing isotopic mass e. none of the above |
a. increasing atomic number
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Which of the following elements are fourth period semimetals?
a. Si and Ge b. Ge and As c. Sb and Te d. Po and At e. none of the above |
b. Ge and As
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Which of the following is a radioactive metal?
a. P b. Pm c. Po d. Pr e. none of the above |
b. Pm
Actually Po (polonium) and Pm (promethium) are both radio-active.. so not sure what it's saying ONLy Pm is the answer. |
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Which of the following is an alkali metal?
a. Al b. Cs c. Cu d. Mg e. none of the above |
b. Cs
Over to the left side of the periodic table are the alkali metals. Then the Earth metals. |
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Which of the following is an alkaline earth metal?
a. Mg b. Ca c. Ba d. all of the above e. none of the above |
d. all of the above
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Which of the following is a halogen?
a. Be b. Br c. H d. Hg e. none of the above |
b. Br
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Which of the following is a noble gas?
a. Au b. Kr c. N d. No e. none of the above |
b. Kr
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Which of the following has the largest atomic radius?
a. Na b. K c. Ca d. Fe e. Al |
b. K
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Which of the following has chemical properties most similar to zinc?
a. Al b. Ga c. Cd d. Ag e. Cu |
c. Cd
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Given the chemical formulas MgO, Al2O3, and SiO2, predict the formula for germanium oxide, Ge?O?.
a. GeO b. Ge2O c. GeO2 d. Ge2O3 e. Ge3O2 |
c. GeO2
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Which energy sublevel is being filled by the elements Ga through Kr?
a. 3d b. 4s c. 4p d. 4d e. 4f |
c. 4p
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What is the core notation for the electron configuration of an iodine atom?
a. [Kr] b. [Kr] 5s2 4p5 c. [Kr] 5s2 4d10 5p5 d. [Kr] 5s2 4d10 5d6 e. [Xe] |
c. [Kr] 5s2 4d10 5p5
So back up to the most recent Noble Gas (Kr in this case) then count the entire next row. Following Kr all the way to Iodine is : KR - 5s, 4d, 5p5... Notice the last digit is only 5. That is the number of squares from the start of the "p" of row 5. There are only 5 from In to I. |
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Predict the number of valence electrons for a Group IIIA/13 element.
a. 2 b. 3 c. 5 d. 8 e. 13 |
b. 3
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Predict the number of valence electrons for a sulfur atom.
a. 4 b. 6 c. 8 d. 16 e. 32 |
b. 6
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Which of the following elements has the lowest ionization energy?
a. K b. Ca c. Rb d. Sr e. Kr |
c. Rb
Rb being the lowest and to the left in periodic table. The lowest and to the left has the lesser energy than say Helium which is far upper right and a gas. |
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Which of the following elements has the highest ionization energy?
a. H b. He c. Ne d. Cl e. F |
b. He
It is far up and to the right and is a gas. |
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Which of the following groups has a predictable ionic charge of one positive?
a. Group IA/1 b. Group IB/11 c. Group IIIA/13 d. Group VIIA/17 tf e. Group VIIIA/18 |
a. Group IA/1
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What is the predicted ionic charge for a S ion?
a. 2+ b. 2– c. 6+ d. 6– e. none of the above |
b. 2–
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Which of the following ions is isoelectronic with the noble gas krypton?
a. As3+ b. I– c. Se2– d. K+ e. none of the above |
c Se2–
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What is the electron configuration for an aluminum ion, Al3+?
a. 1s2 2s2 2p6 because it no longer has 3 electrons. It has 10 = 2+2+6 b. 1s2 2s2 2p6 3s2 c. 1s2 2s2 2p6 3p1 d. 1s2 2s2 2p6 3s2 3p1 e. none of the above |
a
a. 1s2 2s2 2p6 because it no longer has 3 electrons. It has 10 = 2+2+6 |
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What is the electron configuration using core notation for Co3+? (Transition metals 2 of their highest energy s electrons first.)
a. [Ar] b. [Ar] 4s2 3d7 c. [Ar] 4s2 3d4 d. [Ar] 3d6 e. none of the above |
d. [Ar] 3d6
This answer is correct because Co3+ has lost three of it's transition electrons. Thus transition metals loser their 4s's and one 3d thus equalling three. Therefore it would be Fe??? Kind of strange. |
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What is the electron configuration using core notation for I–?
a. [Kr] 5s2 4d10 5p4 b. [Kr] 5s2 4d10 5p5 c. [Kr] 5s2 5p6 d. [Xe] e. none of the above |
d. [Xe]
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