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Questions and Answers
What is the primary characteristic of metals?
What is the primary characteristic of metals?
Which type of element typically gains electrons during chemical reactions?
Which type of element typically gains electrons during chemical reactions?
In which group of the periodic table would you find chlorine?
In which group of the periodic table would you find chlorine?
What is true about metalloids?
What is true about metalloids?
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What type of ion is formed when an atom loses electrons?
What type of ion is formed when an atom loses electrons?
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Which statement about ions is accurate?
Which statement about ions is accurate?
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Which property is NOT typical for nonmetals?
Which property is NOT typical for nonmetals?
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What does the atomic number of chlorine indicate?
What does the atomic number of chlorine indicate?
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What happens to metal atoms in the context of ionic compounds?
What happens to metal atoms in the context of ionic compounds?
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How is the ionic charge represented in chemical symbols?
How is the ionic charge represented in chemical symbols?
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What is the ionic charge of a chlorine ion that has gained one electron?
What is the ionic charge of a chlorine ion that has gained one electron?
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What is the correct formula for an ionic compound formed from Li+ and O2-?
What is the correct formula for an ionic compound formed from Li+ and O2-?
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When the charges on cations and anions are equal, what is the subscript for each ion in the formula for an ionic compound?
When the charges on cations and anions are equal, what is the subscript for each ion in the formula for an ionic compound?
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What is the empirical formula for an ionic compound with a cation of +2 charge and an anion of -1 charge?
What is the empirical formula for an ionic compound with a cation of +2 charge and an anion of -1 charge?
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How are ions in ionic compounds typically arranged?
How are ions in ionic compounds typically arranged?
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Which of the following represents the mass number for an ion with 22 protons and 26 neutrons?
Which of the following represents the mass number for an ion with 22 protons and 26 neutrons?
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What does the empirical formula represent?
What does the empirical formula represent?
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How is electrical neutrality achieved in ionic compounds?
How is electrical neutrality achieved in ionic compounds?
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Which property is characteristic of ionic compounds?
Which property is characteristic of ionic compounds?
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What type of bond forms when electrons are shared between atoms?
What type of bond forms when electrons are shared between atoms?
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What is a diatomic molecule?
What is a diatomic molecule?
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What distinguishes molecular compounds from ionic compounds?
What distinguishes molecular compounds from ionic compounds?
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Which of the following signifies the actual numbers of atoms in a molecule?
Which of the following signifies the actual numbers of atoms in a molecule?
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Why do ionic compounds generally have high melting and boiling points?
Why do ionic compounds generally have high melting and boiling points?
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Study Notes
Metals
- Good conductors of heat and electricity
- Shiny (lustrous)
- Malleable (can be shaped)
- Tend to lose electrons in chemical reactions (form cations)
Nonmetals
- Poor conductors of heat and electricity
- Not shiny (dull)
- Not malleable (brittle)
- Tend to gain electrons in chemical reactions (form anions)
Metalloids
- Properties intermediate between metals and nonmetals
- Can be good or bad conductors of heat and electricity depending on conditions (semiconductors)
Ions
- Atoms or molecules with a net positive or negative charge due to the loss or gain of electrons
- Cations: Positively charged ions
- Anions: Negatively charged ions
Molecules
- Two or more atoms held together by chemical bonds
Ionic Compounds
- Generally formed by metals and nonmetals
- Ions arranged in a 3D structure
- Total positive charge must equal total negative charge
- The net charge of the cation and anion determine the subscript of each element in the compound (e.g., NaCl - charges of 1+ and 1- so subscripts are 1)
Molecular Compounds
- Contain more than one type of atom
- Mostly composed of nonmetals
- Atoms share electrons (covalent bonds)
- Generally have lower melting and boiling points than ionic compounds
Empirical Formulas
- Represent the simplest whole-number ratio of atoms in a compound
- Provide the relative number of atoms of each type in a molecule
- Subscripts are the smallest possible whole numbers
Molecular Formulas
- Indicate the actual number of atoms in a molecule
- Not always the same as empirical formula (e.g., H2O2 (molecular formula) and HO (empirical formula))
Naming Compounds
- Subscripts and superscripts are used to represent specific information about an element in a compound
- Atomic number is written as a subscript on the left of the element symbol
- Mass number is written as a superscript on the left of the element symbol
- Ionic charge is written as a superscript on the right of the element symbol (if charge is 0, nothing is written)
- If the charge is +1 or -1, only the + or - sign is written
- If the charge is +2, +3, -2, or -3, the number followed by the sign is written
Electron Transfer
- Atoms gain or lose electrons to achieve a noble gas configuration (stable electron configuration)
- Example: Sodium (Na) loses one electron to form Na+ (cation) and Chlorine (Cl) gains one electron to form Cl- (anion)
Ionic Bonds
- Electrostatic force of attraction between oppositely charged ions
- Example: Na+ and Cl- form NaCl
Properties of Ionic Compounds
- High melting and boiling points
- Conduct electricity when dissolved in water or molten
Covalent Bonds
- Sharing of electron pairs between atoms
- Example: Water (H2O) formed by sharing electrons between hydrogen and oxygen atoms
Stoichiometry of Compounds
- Empirical and molecular formulas provide information about the ratio and actual number of atoms in a compound
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Description
This quiz covers the properties of metals, nonmetals, and metalloids, including their conductivity, luster, and malleability. Additionally, it explores the characteristics of ions and the formation of ionic compounds. Test your understanding of these fundamental chemistry concepts.
