Chemistry Vocabulary Quiz

Vocabulary

• Isotope: Atoms of the same element that have the same number of protons but a different number of neutrons.
• Cation: An ion that has a positive charge due to the loss of electrons.
• Anion: An ion that has a negative charge due to the gain of electrons.
• Valence Electron: Electrons in the outermost shell of an atom and are responsible for chemical bonding.
• Atomic Number: The number of protons in an atom's nucleus, which defines the element.
• Atomic Mass: The average mass of an atom of an element, taking into account the different isotopes.
• Octet Rule: Atoms tend to gain, lose, or share electrons to achieve a stable configuration of eight electrons in their valence shell.
• Family or Group: A vertical column on the periodic table containing elements with similar chemical properties.
• Period: A horizontal row on the periodic table containing elements with the same number of electron shells.
• Radioactivity: The spontaneous emission of particles or energy from an unstable atomic nucleus.
• Alpha Particle: A positively charged particle consisting of two protons and two neutrons, emitted during radioactive decay.
• Beta Particle: A high-energy electron emitted during radioactive decay.
• Chain Reaction: A self-sustaining series of nuclear fission events, where each fission releases neutrons that trigger further fissions.
• Gamma Ray: A high-energy electromagnetic radiation emitted during radioactive decay.
• Nuclear Fission: The process of splitting a heavy atomic nucleus, releasing energy and neutrons.
• Nuclear Fusion: The process of combining two light atomic nuclei to form a heavier nucleus, releasing energy.
• Half-life: The time it takes for half of the radioactive atoms in a sample to decay.
• Carbon Dating: A technique for determining the age of ancient artifacts and fossils by measuring the ratio of carbon-14 to carbon-12.

Patterns on the Periodic Table

• Atomic Number: Increases from left to right and top to bottom.
• Atomic Mass: Generally increases from left to right and top to bottom.
• Electronegativity: Increases from left to right and bottom to top.
• Ionization Energy: Increases from left to right and bottom to top.
• Metallic Character: Decreases from left to right and increases from top to bottom.

Valence Electrons

• Determined by the group number of an element on the periodic table (except for transition metals).

Nuclear Reactors

• Negatives:
  • Production of radioactive waste.
  • Risk of accidents (e.g., Chernobyl, Fukushima).
  • Proliferation of weapons-grade materials.
• Positives:
  • Carbon-free electricity generation.
  • High energy output.
  • Relatively low operating costs.

Noble Gases

• Unreactive because they have a full outer shell of electrons (8 electrons for most, except Helium with 2).

Electron Energy Levels

• First Energy Level: Maximum 2 electrons.
• Second Energy Level: Maximum 8 electrons.
• Third Energy Level: Maximum 18 electrons.

Families or Groups in Periodic Table

• All elements in a given group have the same number of valence electrons.

Nitrogen Atom, Isotope, and Ion

• Atom: 7 protons, 7 neutrons, 7 electrons.

• Isotope: 7 protons, 8 neutrons, 7 electrons.

• Ion: 7 protons, 7 neutrons, 10 electrons.

• The number of neutrons and electrons differentiate between isotopes and ions, respectively.

Carbon-14 Radioactivity

• Carbon-14 has 6 protons and 8 neutrons. The unstable ratio of protons to neutrons makes it radioactive.

Oxygen Model

• Neutral: 8 protons, 8 neutrons, 8 electrons.
• Anion: 8 protons, 8 neutrons, 10 electrons.

Losing Valence Electrons

• Losing two valence electrons forms a +2 cation.

Neighboring Atoms on Periodic Table

• The primary difference between two neighboring atoms horizontally on the periodic table is their number of protons (atomic number) and valence electrons.

Top and Bottom Neighbors on Periodic Table

• The primary difference between two neighboring atoms vertically on the periodic table is the number of electron shells and their energy levels.

Chromium-63

• Chromium-63 has 27 protons and 36 neutrons (63 - 27 = 36).

Hydrogen Isotopes

• Hydrogen -1: 1 proton, 0 neutrons, 1 electron (Protium)
• Hydrogen -2: 1 proton, 1 neutron, 1 electron (Deuterium)
• Hydrogen -3: 1 proton, 2 neutrons, 1 electron (Tritium)

Mystery Elements

• Good Conductor: Likely located in the left side of the periodic table, in the metal section.
• Semiconductor: Likely found in the metalloid section of the periodic table (border between metals and nonmetals).
• Poor Conductor: Likely found in the right side of the periodic table, in the nonmetal section.

Unstable Isotopes

• Undergo radioactive decay to become more stable.

Nuclear Energy Arguments

• For:
  • Low-carbon energy source.
  • High energy yield compared to other sources.
  • Relatively low operating costs.
• Against:
  • Production of radioactive waste.
  • Risk of accidents.
  • Proliferation of weapons-grade materials.

Nuclear Fission Process

• A heavy atom (such as uranium) is bombarded with a neutron, causing it to split into two or more lighter atoms.
• This process releases energy and additional neutrons that trigger further fission reactions.

Fusion in the Sun

• The process of nuclear fusion powers the Sun, where hydrogen nuclei fuse to form helium nuclei, releasing immense energy.

Elements Likely to Undergo Fusion

• Light elements, such as hydrogen, helium, and lithium.

Elements Likely to Undergo Fission

• Heavy elements, such as uranium, thorium, and plutonium.

Graphics Conclusions

• (Please provide the graphics for me to conclude)

Test your knowledge of essential chemistry terms and concepts. This quiz covers important vocabulary such as isotopes, cations, anions, and more, that are fundamental to understanding atomic structure and chemical bonding. Perfect for students looking to reinforce their understanding of chemistry.