SCI9_SEATWORK: VALENCE ELECTRONS AND BOND FORMATION

Dots are often used to represent the valence electrons in atoms and molecules. The resulting structures are referred to as ______________________________.

• Light emitting diode structures

• Lewis electron-dot structures

• London dispersion forces

• Light electron diode structures

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What is the principle that governs bonding, and how do certain elements differ in their adherence to this principle?

• Bonding follows the duet rule, where atoms aim to have two outer electrons, while elements such as lithium, helium, hydrogen, and beryllium adhere to the octet rule.

• Bonding follows the octet rule, where atoms aim to have eight outer electrons, while elements such as lithium, helium, hydrogen, and beryllium obey the duet rule.

• Bonding follows the duet rule, where atoms aim to have eight outer electrons, while elements such as lithium, helium, hydrogen, and beryllium adhere to the octet rule.

• Bonding follows the octet rule, where atoms aim to have two outer electrons, while elements such as lithium, helium, hydrogen, and beryllium obey the octet rule.

How do atoms combine to form an ionic bond?

• Atoms combine through the sharing of electrons.

• Atoms combine through the transfer of protons.

• Atoms combine through the transfer of neutrons.

• Atoms combine through the transfer of electrons.

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How do atoms combine to form a metallic bond?

• Atoms combine through the transfer of electrons.

• Atoms combine through the sharing of neutrons.

• Atoms combine through the overlap of orbitals.

• Atoms combine through the sharing of protons.

How do atoms combine to form a covalent bond?

• Atoms combine through the sharing of electrons.

• Atoms combine through the sharing of neutrons.

• Atoms combine through the sharing of protons.

• Atoms combine through the transfer of electrons.

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In ionic bonding, what is the general behavior of metal atoms regarding the loss of electrons, and how does it relate to specific groups?

• Metal atoms gain electrons, and Groups 1A, 2A, and 3A can gain a maximum of 1, 2, and 3 electrons, respectively.

• Metal atoms lose protons, and Groups 1A, 2A, and 3A can lose a maximum of 1, 2, and 3 protons, respectively.

• Metal atoms lose electrons, and Groups 1A, 2A, and 3A can lose a maximum of 1, 2, and 3 electrons, respectively.

• Metal atoms gain protons, and Groups 1A, 2A, and 3A can gain a maximum of 1, 2, and 3 protons, respectively.

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In ionic bonding, what is the general behavior of nonmetal atoms regarding the gain of electrons, and how does it relate to specific groups?

• Nonmetal atoms gain electrons, and Groups 5A, 6A, and 7A can gain 3, 2, and 1 electron(s), respectively.

• Nonmetal atoms lose electrons, and Groups 5A, 6A, and 7A can lose 3, 2, and 1 electron(s), respectively.

• Nonmetal atoms lose protons, and Groups 5A, 6A, and 7A can lose 3, 2, and 1 proton(s), respectively.

• Nonmetal atoms gain protons, and Groups 5A, 6A, and 7A can gain 3, 2, and 1 proton(s), respectively.

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What is the term for a charged particle formed when a neutral atom gains or loses an electron, and how are positive and negative ions classified?

• A compound; positive ions are cations, and negative ions are anions.

• An ion; positive ions are cations, and negative ions are anions.

• A molecule; positive ions are anions, and negative ions are cations.

• An isotope; positive ions are anions, and negative ions are cations.

In ionic compounds, how are cations and anions balanced, and how do nonmetals contribute to the charge balance?

• Cations are balanced by protons, and nonmetals complement metals by forming positive ions.

• Cations are balanced by electrons, and nonmetals complement metals by forming positive ions.

• Cations are balanced by anions, and nonmetals complement metals by forming negative ions.

• Cations are balanced by neutrons, and nonmetals complement metals by forming negative ions

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What does the term "valence" refer to, and which electrons in an atom are specifically called valence electrons?

• Valence refers to the capacity of atoms to form bonds; the electrons in the outermost energy level are valence electrons.

• Valence refers to the capacity of atoms to form bonds; all electrons in the innermost energy level are valence electrons.

• Valence refers to the total number of energy levels in an atom; all electrons in the outermost energy level are valence electrons.

• Valence refers to the total number of electrons in an atom; all electrons are considered valence electrons.

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