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Questions and Answers
What happens to the valence electrons of a metal when it combines with a non-metal?
What happens to the valence electrons of a metal when it combines with a non-metal?
The valence electrons of the metal are transferred to the valence shell of the non-metal.
What is formed when an atom loses a valence electron?
What is formed when an atom loses a valence electron?
An ion.
What charge does a cation have?
What charge does a cation have?
Positive charge.
Which of the following ions are isoelectronic with Ne?
Which of the following ions are isoelectronic with Ne?
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What charge does an anion have?
What charge does an anion have?
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A cation is formed by the ____ of electrons.
A cation is formed by the ____ of electrons.
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Which groups typically form cations?
Which groups typically form cations?
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An anion is formed by the ____ of electrons.
An anion is formed by the ____ of electrons.
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Which of the following correctly represents cation formation from calcium?
Which of the following correctly represents cation formation from calcium?
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Which of the following ions is produced when an oxygen atom gains electrons?
Which of the following ions is produced when an oxygen atom gains electrons?
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Ionic compounds are held together by ____ forces.
Ionic compounds are held together by ____ forces.
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Study Notes
Atoms
- Atomic structure consists of protons, neutrons, and electrons.
- Atomic weight refers to the average mass of an element's isotopes.
- Atomic number denotes the number of protons in an atom, defining the element.
- Isotopes are variants of an element with the same number of protons but different numbers of neutrons.
The Periodic Table
- Electron configuration describes the distribution of electrons in an atom's orbitals.
- Elements are arranged in groups (vertical columns) and periods (horizontal rows) based on their properties.
- Trends include ionization energy, electronegativity, and atomic radius, varying across periods and groups.
Molecules and Molecular Compounds
- Molecules form when two or more atoms share electrons through covalent bonding.
- Molecular compounds typically consist of non-metals bonded together.
Ions and Ionic Compounds
- Ionic compounds form when metals donate valence electrons to non-metals.
- Example: Calcium transfers electrons to chlorine, forming Ca2+ and Cl- ions.
- Ion formation helps atoms achieve electronic configurations similar to noble gases.
Ion Formation
- Ions develop when atoms gain or lose electrons; a neutral atom has equal protons and electrons.
- Cations are formed by metals losing electrons (e.g., Ca → Ca2+).
- Anions form when non-metals gain electrons (e.g., Cl + e- → Cl-).
Group-Specific Ion Formation
- Group 1 and 2 elements typically form M+ and M2+ ions (e.g., Na+, Ca2+).
- Group 13 elements form M3+ ions (e.g., Al3+).
- Group 15 elements form X3- ions (e.g., N3-).
- Group 16 elements form X2- ions (e.g., O2-, S2-).
- Transition metals can form variable ions (e.g., Cu+, Cu2+).
Ionic Compounds Characteristics
- Ionic compounds consist of cations and anions held together by electrostatic forces.
- After losing electrons, metals become positively charged (more protons than electrons).
- Non-metals gain electrons to become negatively charged (more electrons than protons).
- The attraction between oppositely charged ions leads to the formation of ionic bonds.
Example Equations for Ion Formation
- Formation of N3-: N + 3e- → N3-
- Formation of O2-: O + 2e- → O2-
- Formation of F-: F + e- → F-
- Formation of Na+: Na → Na+ + e-
- Formation of Mg2+: Mg → Mg2+ + 2e-
- Formation of Al3+: Al → Al3+ + 3e-
Summary of Ionic Bonding Process
- When a metal loses electrons, it forms a cation (e.g., Ca → Ca2+).
- When a non-metal gains electrons, it forms an anion (e.g., O + 2e- → O2-).
- The resulting cation and anion attract each other, forming stable ionic compounds.
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Description
This quiz covers essential concepts of atoms, molecules, and ions, including atomic structure, the periodic table, and bonding types. You'll explore topics such as electron configuration, isotope differences, and trends within the periodic table. Test your knowledge of covalent and ionic compounds in this comprehensive assessment.
