Unit 6 Assessment

How do main group elements form ions?

• All main group elements lose electrons to form cations.

• All main group elements gain electrons to from anions.

• They lose or gain electrons to achieve a half-filled p or d orbital

• They lose or gain electrons to obtain a noble-gas electron configuration.

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Which ion has a +3 charge and the electron configuration: 1s²2s²2p⁶?

• B³⁺

• Al³⁺

• P³⁺

• Fe³⁺

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Chlorine and potassium will both ionize to achieve the same electron configuration as which noble gas?

• He

• Ne

• Ar

• Kr

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Which of the following best describes the Born-Haber cycle?

• The cycle explains the energy change that occurs when an electron is added to an atom.

• The cycle gives the mathematical relationship between charge interaction and energy.

• The cycle identifies the amount of energy required to remove the outermost electron from an isolated atom.

• The cycle is a series of hypothetical steps, used to analyze the overall energy change during the formation of an ionic compound.

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What is the term for the electrons involved in the formation of a chemical bond?

• Lewis electrons

• core electrons

• excited electrons

• valence electrons

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Which element which exhibits the greatest electronegativity?

• O

• F

• Fr

• S

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Which of the following ions is NOT isoelectronic with neon?

• O^2-

• Ca²⁺

• Al³⁺

• Mg²⁺

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What happens to the lattice energy as the distance between ions increases in a crystal?

• Lattice energy increases

• Lattice energy decreases

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Which of the following is true concerning lattice energies?

• Lattice energy is always negative.

• Lattice energy is always positive.

• Lattice energy is large when the distance between ions is large.

• Lattice energy is a measure of molecular strength.

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Main group elements commonly undergo chemical reactions. Which of the following best describes the electron arrangement for main group elements after the chemical reaction has occured.

• The elements have eight inner shell (core) electrons.

• The elements have eight outer shell (valence) electrons.

• The elements have less stable electron arrangements.

• The elements have electrons in excited states.

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