Atomic Structure and Isotopes Quiz
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Atomic Structure and Composition

  • The nucleus of an atom contains protons and neutrons.
  • Electrons orbit the nucleus.
  • Protons have a positive charge.
  • Neutrons have no charge.
  • Electrons have a negative charge.
  • Potassium is a metal.
  • Chlorine is a nonmetal.
  • Aluminum and sulfur form the ionic compound Al₂S₃.

Chemical Formulas and Naming

  • The correct name for SrO is strontium oxide.
  • The name for PCl₃ is phosphorus trichloride.
  • The formula for ammonium carbonate is (NH₄)₂CO₃.

Subatomic Particles

  • The smallest and lightest subatomic particle is the electron.
  • Isotopes have the same number of protons but different numbers of neutrons.
  • Argon-18 has 18 electrons, 18 protons and 22 neutrons.

Isotopes and Atomic Mass

  • Isotopes have the same number of protons but different numbers of neutrons.
  • An element's average atomic mass is the weighted average of the masses of its isotopes.
  • For Si, the average atomic mass is 28.10 amu.

Electromagnetic Radiation

  • The wavelength of light with a frequency of 1.20 x 10³¹ s⁻¹is 2.50 x 10⁻⁵ m.
  • The frequency of electromagnetic radiation with a wavelength of 0.53 m is 5.7 x10⁸ s⁻¹.

Quantum Numbers

  • Electron quantum numbers are used to describe an electron in an atom (a, b and c).
  • An electron cannot have certain quantum numbers, (d).
  • Examples of valid electron quantum numbers are (e).

Electron Configurations

  • The electron configuration for nitrogen is 1s²2s²2p³.
  • The ground state electron configuration for Zinc is [Ar] 4s²3d¹⁰.
  • The largest principal quantum number in the ground state electron configuration of barium is 6.
  • Atomic radius generally increases down a group and decreases across a period.
  • First ionization energies generally increase across a period and decrease down a group.

Chemical Bonding

  • Ionic compounds form when electrons are transferred between atoms.
  • Molecular compounds form when electrons are shared between atoms.
  • The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full outer electron shell.
  • Bromine (Br₂) forms molecular compounds.
  • Strontium (Sr²⁺) typically forms ionic bonds.
  • Examples of isoelectronic series are (O², F⁻, Ne, Na⁺).
  • The Lewis structure of water shows 2 nonbonding electron pairs on the oxygen atom.

Other Concepts

  • There are 9 orbitals in the third shell.
  • The lowest-energy shell that contains f orbitals is the n = 5 shell.
  • Four quantum numbers are needed to define an electron in an atom.
  • The most common ion of Sulfur (S) has a charge of 2⁻.

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Fall 2024 Chemistry Midterm PDF

Description

Test your knowledge on atomic structure, the composition of atoms, subatomic particles, and isotopes. This quiz will cover key concepts including the properties of protons, neutrons, electrons, and how to correctly name and write chemical formulas. Prepare to demonstrate your understanding of atomic mass and formulas!

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