Atomic Structure and Electrons Quiz

Study Notes

Subatomic Particles

Electrons (e-) are negatively charged, have a mass of approximately 9.109 x 10⁻²⁸ grams, and make up the electron cloud surrounding the nucleus.
Protons (p+) carry a positive charge and have a mass of 1.673 x 10⁻²⁴ grams with a relative mass of 1.0073 amu; they define the atomic number of an element.
Neutrons (n0) are neutral particles, discovered by James Chadwick, with a mass of about 1.0087 amu; they play a crucial role in the stability of the nucleus.

Atomic Structure

Atoms consist of a dense nucleus containing protons and neutrons, surrounded by electrons in motion.
The atomic theory, initiated by Democritus, emphasizes that all matter is composed of atoms.
The Bohr model illustrates how electrons occupy defined energy levels around the nucleus.

Molecular Types

Homonuclear molecules are formed from one kind of element (e.g., O₂).
Heteronuclear molecules consist of multiple elements (e.g., H₂O).

Chemical Bonding

Ionic bonds form between metals and nonmetals through electron transfer, resulting in positively charged cations and negatively charged anions.
Covalent bonds involve sharing electron pairs between atoms; critical for the formation of molecules.
Hydrogen bonds are weak non-covalent interactions significant in molecular interactions.

Isotopes

Isotopes are variants of the same element that have different numbers of neutrons, affecting atomic stability.

Periodic Table Trends

Elements are arranged by atomic number, leading to periodic trends in properties such as density, atomic radius, and ionization energy.
Nonmetals typically gain electrons (forming anions), while metals tend to lose electrons (forming cations) based on their valence electron configuration.

Reactivity

Non-metal reactivity increases as elements more easily gain electrons to achieve a stable electronic configuration.
Metal reactivity is assessed by their ability to lose electrons; less energy is required for those with fewer valence electrons.

Ionization Energy and Electronegativity

Ionization energy measures the energy required to remove the outermost electron from a gaseous atom, with non-metals exhibiting higher ionization energies.
Electronegativity, measured in Pauling units, indicates an atom's ability to attract electrons in a bond, with fluorine being the most electronegative element.

Chemical Names and Formulas

Ionic compounds consist of metal and non-metal ions, typically latticed with loose attachment.
In naming binary ionic compounds, the cation is named first followed by the anion name, modified to end in "ide."

Allotropes

Elements can exist in different structural forms (allotropes) even in the same phase, such as graphite and diamond, both of which are forms of carbon.

Description

Test your knowledge on atomic structure, particularly focusing on electrons, atomic numbers, and their associated masses. This quiz covers key concepts and facts related to the fundamental building blocks of matter. Perfect for students learning about chemistry and atomic theory.