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Questions and Answers
Which of the following accurately describes an isotope?
Which of the following accurately describes an isotope?
- Atoms with different numbers of protons and electrons.
- Atoms of the same element with different atomic masses. (correct)
- Atoms with unequal numbers of neutrons and electrons.
- Atoms that cannot exist in nature.
What is the defining characteristic of an ionic bond?
What is the defining characteristic of an ionic bond?
- It occurs between atoms of the same type.
- It involves the attraction between ions of opposite charges. (correct)
- It involves the sharing of electrons between nonmetals.
- It is formed solely between metals.
Which of the following is a characteristic of a molecule?
Which of the following is a characteristic of a molecule?
- It has the same properties as its constituent atoms.
- It can consist of just one type of atom.
- It must contain more than two atoms.
- It consists of atoms that are chemically bonded. (correct)
Which statement correctly defines a compound?
Which statement correctly defines a compound?
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What does an electron dot formula represent?
What does an electron dot formula represent?
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What is characteristic of a double bond between two atoms?
What is characteristic of a double bond between two atoms?
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Which statement accurately describes a molecular formula?
Which statement accurately describes a molecular formula?
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What occurs during the reduction process in ionic compounds?
What occurs during the reduction process in ionic compounds?
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Which of the following correctly defines isomers?
Which of the following correctly defines isomers?
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What distinguishes organic compounds from inorganic compounds?
What distinguishes organic compounds from inorganic compounds?
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Study Notes
Chemical Bonds
- Double Bond: Atoms share two pairs of electrons; example: ethylene (C2H4).
- Triple Bond: Atoms share three pairs of electrons; example: nitrogen (N2).
Chemical Formulas
- Structural Formula: Illustrates atomic arrangement and shared electrons; example: hydrogen sulfide (H2S).
- Molecular Formula: Indicates quantity of atoms in a molecule; example: two moles of carbon dioxide (2 CO2).
Oxidation and Reduction
- Oxidation (Ionic): Involves loss of electrons; example: sodium ion formation (Na → Na+ + e).
- Reduction (Ionic): Involves gain of electrons; example: fluoride ion formation (F + e- → F).
- Oxidation (Covalent): Involves loss of hydrogen atoms; results in an increase in oxidation state.
- Reduction (Covalent): Involves gain of hydrogen atoms; leads to a decrease in oxidation state.
Isomers
- Defined as molecules with identical formulas but distinct structural arrangements or spatial orientations; example: glucose (C6H12O6).
Types of Compounds
- Organic Compounds: Chemical substances that contain carbon; example: heptane (C7H16).
- Inorganic Compounds: Compounds not based on carbon, except CO and CO2; example: potassium chloride (KCl).
Atomic Structure
- Atom: Smallest unit of matter, indivisible by chemical means; example: helium atom consisting of 2 electrons (e), 2 protons (p), and 2 neutrons (n).
- Element: Pure substance comprising one type of atom; example: gold (Au).
- Isotope: Atoms with the same number of protons and electrons but differing in neutrons, leading to varying atomic mass; examples: Carbon-12 (6 e, 6 p, 6 n) and Carbon-13 (6 e, 6 p, 7 n).
Ions
- Ion: Atom or group of atoms with a charge, either positive or negative; example: sodium ion (Na+; 11 p, 12 n, 10 e).
Bonds
- Ionic Bond: Attraction between oppositely charged ions, typically between metals and non-metals.
- Covalent Bond: Attraction resulting from the sharing of electrons between nonmetal atoms; example: water (H2O).
Molecules and Compounds
- Molecule: Smallest unit where atoms are chemically bonded; retains properties of the compound; example: diatomic hydrogen (H2).
- Compound: Substances made up of more than one type of atom joined together; example: hydrogen fluoride (HF).
Electron Dot Formula
- Visualization technique representing valence electrons; dots indicate electrons in outer shells; example: neon (Ne).
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