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63 Cards in this Set
- Front
- Back
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Any member of a group of gaseous elements in Group 0 of the period table; the s and p sublevels of their outermost energy level are filled. |
Noble gases
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Group A element on the periodic table; together, these elements, which have only partially filled outermost s and p sublevels, illustrate the entire range of chemical properties.
What is it? |
Representative element
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Define Transition Metal.
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Called Group B elements and are characterized by addition of electrons to the d orbital
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Define Inner Transition Metal.
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Characterized by the filling of f orbitals; an element in the lanthanide and actinide series.
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Define Atomic Radius.
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1/2 of the distance between the nuclei of two like atoms in a diatomic molecule
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The tendency for an atom to attract electrons to itself when it is chemically combined with another element.
What is it? |
Electronegativity
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Define Ionization Energy.
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The energy required to remove an electron from a gaseous state.
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Which group of the periodic table has the highest electronegativity?
A) 6A B) 7A C) 2A D) 1A E) 3A |
B) 7A
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How does the shielding phenomenon affect the relative atomic sizes of elements in the same period?
A) An increase in the degree of shielding causes a decrease in atomic size. B) Shielding has no effect on relative atomic size within a period. C) An increase in the degree of shielding causes an increase in atomic size. |
B) Shielding has no effect on relative atomic size within a period.
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The representative elements are usually called...
A) halogens B) Group B elements C) Group A elements D) noble gases |
C) Group A elements
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Why is the radius of a positive ion always less than the radius of its neutral atom?
A) The nucleus pulls the remaining electrons in closer. B) The atomic orbitals contract all by themselves. C) Electron speeds are reduced. D) The number of principal energy levels is always reduced. |
A) The nucleus pulls the remaining electrons in closer.
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Which of the following factors contributes to the lower ionization energy of the higher-atomic-number elements in a family in the periodic table?
A) greater distance from nucleus B) greater number of protons in nuclei C) smaller number of valence electrons D) larger nuclei |
A) greater distance from nucleus
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Which of the following elements, when ionically bound to sulfur, attracts electrons less strongly than the sulfur?
A) fluorine B) oxygen C) cesium D) chlorine |
C) cesium
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Compared with the electronegativities of the elements at the left end of a particular period, the electronegativities of the elements at the right side of that same period tend to be...
A) unpredictable B) the same C) lower D) higher |
D) higher
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Why is the radius of a negative ion always greater than the radius of its neutral atom?
A) because the number of principal energy levels is always reduced B) because atomic orbitals contract all by themselves C) because repulsion between electrons increases D) because electron speeds are reduced |
C) because repulsion between electrons increases
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For Group 2A metals, which electron is the most difficult to remove from a neutral atom?
A) the second B) the first C) the third D) All the electrons are equally difficult to remove. |
C) the third
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What is the electron configuration of sulfur?
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1s^2 2s^2 2p^6 3s^2 3p^4
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Which of the following elements has the lowest electronegativity?
A) carbon B) bromine C) lithium D) fluorine |
C) lithium
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What orbital is filled when iodine gains an electron to become a negative ion?
A) 4d B) 5p C) 4p D 6s |
B) 5p
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Which of the following elements has the smallest atomic radius?
A) S B) O C) Li D) K |
B) O
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The energy required to remove an electron from a gaseous atom is called the...
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ionization energy
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Which of the following factors contributes to the relatively greater atomic size of the higher-atomic-number elements within a particular family of the periodic table?
A) smaller number of valence electrons B) larger nuclei C) more shielding of the outer electrons by the inner electrons D) greater number of protons |
C) more shielding of the outer electrons by the inner electrons
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Atomic size generally...
A) remains constant within a period B) increases as you move from left to right across a period C) decreases as you move from left to right across a period D) decreases as you move down a group |
C) decreases as you move from left to right across a period
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How does atomic radius change from left to right across a period in the periodic table?
A) It tends to decrease. B) It first decreases, then increases. C) It does not change. D) It first increases, then decreases. E) It tends to increase. |
A) It tends to decrease.
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What is true of the electron configurations of the noble gases?
A) The outermost s and f sublevels are very close in energy and have electrons in them. B) The outermost s and p sublevels are partially filled. C) The outermost s and p sublevels are filled. D) The outermost s and d sublevels are very close in energy and have electrons in them. |
C) The outermost s and p sublevels are filled.
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Of the following atoms, which one has the smallest first ionization energy?
A) aluminum B) boron C) silicon D) carbon |
A) aluminum
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Atomic radii generally decrease as you move from left to right in a given period because there is...
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increase in the nuclear charge
# of inner electrons--shielding effect--remains constant |
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Ionization energy (A)_____ as you move from left to right across a period. It (B)_____ as you move down a group.
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(A) increases
(B) decreases |
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Define Valence Electron.
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An electron in the highest occupied energy level of an atom.
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A notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus; also called Lewis dot structures.
What is it? |
Electron dot structure
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Atoms react by losing or gaining electrons to acquire stable electron structure of a noble gas, usually 8 valence electrons.
What is it? |
Octet Rule
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Define Halide Ion.
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A negative ion formed when a halogen atom gains an electron.
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Define Ionic Bond.
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the electrostatic attraction that binds oppositely charged ions together
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Define Coordination Number.
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the number of ions of opposite charge that surround each ion in a crystal.
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The force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions.
What is it? |
Metallic Bond
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What is the formula for potassium sulfide?
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K2S
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Which of the following is a pseudo-noble-gas electron configuration?
A) 1s^2 2s^2 2p^6 3s^2 3d^10 3f^14 B) 1s^2 2s^2 2p^6 3s^2 3d^5 C) 1s^2 2s^2 2p^6 3s^2 3d^6 D) 1s^2 2s^2 2p^6 3s^2 3d^10 E) 1s^2 2s^2 2p^6 3s^2 3d^10 4s^2 |
D) 1s^2 2s^2 2p^6 3s^2 3d^10
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How many valence electrons are there in an atom of magnesium?
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2
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What is the formula of the ion formed when cadmium achieves a pseudo-noble-gas electron configuration?
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Cd^2+
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How was the coordination number determined for the oxide ion in rutile (titanium oxide)?
A) by gamma ray diffraction B) by x-ray diffraction C) by infrared spectroscopy D) by ultraviolet spectroscopy E) by ultrasound refractometry |
B) by x-ray diffraction
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How many valence electrons are there in an atom of phosphorus?
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5
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A metallic bond is a bond between...
A) valence electrons and positively charged metal ions B) a metal and a nonmetal C) the ions of two different metals D) none of the above |
A) valence electrons and positively charged metal ions
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The melting temperature of potassium chloride is relatively...
A) low B) Potassium chloride does not melt. C) variable D) high |
D) high
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What is the formula for magnesium sulfide?
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MgS
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Which of the following elements does NOT have an ionic charge of 1+?
A) hydrogen B) potassium C) sodium D) fluorine |
D) fluorine
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Which of the following particles are free to drift in metals?
A) electrons B) protons C) neutrons D) cations E) pions |
A) electrons
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What is the electron configuration of the gallium ion?
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1s^2 2s^2 2p^6 3s^2 3p^6 3d^10
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What is the formula unit of aluminum oxide?
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Al2O3
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What is the charge on the strontium ion?
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2+
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How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound, potassium nitride?
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0
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How many electrons does boron have to give up in order to achieve a noble-gas electron configuration?
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3
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How many electrons does barium have to give up to achieve a noble-gas electron configuration?
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2
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Which of the following ions has a pseudo-noble-gas electron configuration?
A) Fe2+ B) Cu+ C) Mn2+ D Ni+ |
B) Cu+
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What is the net charge of the ionic compound, calcium fluoride?
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0
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does oxygen obey the octet rule when reacting to form compounds?
A) It does not change its number of electrons. B) It gains electrons. C) It gives up electrons. |
B) It gains electrons.
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A compound held together by ionic bonds is called a _____.
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salt
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Which of the following electron configurations is particularly stable?
A) a filled principal energy level B) a filled energy sublevel C) one empty and one filled energy sublevel D) a half-filled energy sublevel |
A) a filled principal energy level
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What characteristic of metals makes them good electrical conductors?
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They have mobile valence electrons.
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What is the formula unit of sodium nitride?
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Na3N
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What is shown by the structural formula of a molecule or polyatomic ion?
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the arrangement of bonded atoms
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What is the charge on the cation in the ionic compound, sodium sulfide?
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1+
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What is the charge of a particle having 9 protons and 10 electrons?
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1-
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Which kind of ion does sulfur become when it combines with a metal?
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anion
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