Questions and Answers
What is defined as the smallest unit of matter that cannot be divided by chemical means?
What is true about isotopes?
Which of the following correctly describes a covalent bond?
What defines an ion?
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What type of bond involves the sharing of three pairs of electrons between two atoms?
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What is a molecule?
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Which formula represents the number of atoms in a molecule without showing their arrangement?
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What does oxidation represent in ionic reactions?
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Which of the following describes molecules that have the same molecular formula but different structural arrangements?
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What term is used for a chemical compound not based on carbon, except for carbon oxides?
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Study Notes
Atom
- Smallest unit of matter, indivisible by chemical means.
- Example: Helium atom with 2 electrons (e-), 2 protons (p+), and 2 neutrons (n or n°).
Element
- Substance consisting of only one type of atom.
- Example: Gold.
Isotope
- Atoms that have the same number of protons and electrons but differ in neutrons and atomic mass.
- Example: Carbon-12 (6 e-, 6 p+, 6 n) vs. Carbon-13 (6 e-, 6 p+, 7 n).
Ion
- Atom or group of atoms that carries a positive or negative charge.
- Example: Sodium ion (Na+) has 11 p+, 12 n, and 10 e-.
Ionic Bond
- Attraction between positively and negatively charged ions, typically between metals and non-metals.
Covalent Bond
- Attraction between nonmetal atoms that occurs due to shared electrons.
Molecule
- A chemical entity where atoms are bonded together retaining compound properties.
- Examples: H2O (water) and H2 (hydrogen gas).
Compound
- Substance containing more than one type of atom bonded together.
- Example: Hydrogen fluoride (HF).
Electron Dot Formula
- Representation using dots to illustrate electrons in outer shells.
- Example: Neon.
Bond Types
- Double Bond: Two pairs of shared electrons between two atoms. Example: Ethylene (C2H4).
- Triple Bond: Three pairs of shared electrons between two atoms. Example: Nitrogen gas (N2).
Chemical Representations
- Structural Formula: Depicts shared electron pairs with lines, showing arrangement of atoms. Example: Hydrogen sulfide (H2S).
- Molecular Formula: Indicates total number of atoms in a molecule. Example: 2 CO2 (two carbon dioxide molecules).
Oxidation and Reduction in Ionic Reactions
- Oxidation: Loss of electrons. Example: Sodium (Na) loses electron to form Na+.
- Reduction: Gain of electrons. Example: Fluorine (F) gains electron to become F-.
Oxidation and Reduction in Covalent Reactions
- Oxidation: Loss of hydrogen atoms, equivalent to losing negative charge.
- Reduction: Gain of hydrogen atoms.
Other Chemical Concepts
- Isomer: Different molecules that share the same formula but vary in bonding or spatial arrangement. Example: Glucose (C6H12O6).
- Organic Compound: Chemical compound primarily containing carbon. Example: Heptane (C7H16).
- Inorganic Compound: Compound not primarily based on carbon, with exceptions like CO and CO2. Example: Potassium chloride (KCl).
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Description
Test your understanding of key chemistry definitions, including atom, element, and isotope. This quiz will help reinforce your knowledge of fundamental concepts in chemistry. Perfect for students looking to review essential terminology.
