Periodic Table, Atomic Structure, and Chemical Bonding Review

Vocabulary practice flashcards covering atomic number, isotopes, ionic versus covalent bonding, electron shell configurations, and periodic trends based on the lecture quiz review.

Strontium Protons vs. Cesium Shells Comparison

A comparison where the number of protons in Strontium ($38$) is greater than ($>$) the total energy levels or electron shells of Cesium (Period $6$).

Barium Ion ($Ba^{2+}$) Electron Count

An ion configuration with $54$ total electrons and $8$ valence electrons, formed from neutral Barium with atomic number $56$.

Nonmetal Ion Behavior

The tendency of nonmetals on the right side of the periodic table to gain valence electrons in order to form negative anions.

Bromide Ion ($Br^-$) vs. Krypton ($Kr$) Comparison

A relationship where the number of electrons in a $Br^-$ ion ($36$) is equal to ($=$) the number of protons in a neutral Krypton atom ($36$).

Silicon Tetrahydride ($SiH_4$)

The covalent compound formula formed between Silicon ($Si$) and Hydrogen ($H$).

Magnesium ($Mg$) Neutral Atom

The neutral element containing $12$ total electrons arranged as $2$ in the first shell, $8$ in the second shell, and $2$ in the third shell.

Isotope Property Variation

The specific subatomic difference between isotopes of an element, such as Nitrogen-$14$ and Nitrogen-$15$, which is a change in the count of neutrons.

Phosphide Ion ($P^{3-}$)

The stable anion formed when a phosphorus atom with $15$ protons gains $3$ electrons.

Aluminum ($Al$) Neutral Element

The original neutral element with $13$ protons that, upon losing $3$ electrons, is left with $10$ electrons remaining (the same electron count as Neon).

Chloride Ion ($Cl^-$) Electron Arrangement

The electron arrangement of $2, 8, 8$ resulting when a chlorine atom (atomic number $17$) gains $1$ electron.

Sodium ($Na$) and Potassium ($K$) Bonding Incompatibility

The inability of Sodium and Potassium to form an ionic compound because both are metals that want to lose electrons to form positive ions.

Chlorine-$35$ Natural Abundance

The more abundant isotope of chlorine in nature because the average atomic mass of $35.45\,\text{amu}$ is closer to $35$ than to $37$.

Calcium Ion ($Ca^{2+}$) vs. Chlorine ($Cl$) Comparison

A comparison where the number of electrons in a $Ca^{2+}$ ion ($18$ electrons) is greater than ($>$) the number of protons in a neutral Chlorine atom ($17$ protons).

Lead ($Pb$) Electron Distribution

A neutral Lead atom (atomic number $82$, Group $14$) characterized by having $82$ total electrons and $4$ valence electrons.

Magnesium and Phosphorus Ionic Combination

The chemical pairing of Magnesium ($Mg^{2+}$) cations and Phosphorus ($P^{3-}$) anions to produce a neutral, balanced ionic compound formula.

Down-Group Shell Trend

The periodic trend where moving down a column/group (such as Lithium to Sodium to Potassium) causes the number of filled electron shells to increase.

Proton Invariance During Ionization

The principle that when an atom gains electrons to form an anion, its number of protons remains completely unchanged.

Aluminum Ion ($Al^{3+}$) Electron Arrangement

The electron arrangement of $2, 8$ for an aluminum ion that has lost $3$ electrons from its neutral atomic number of $13$.

Covalent vs. Ionic Bonding Electron Behavior

The distinction in bonding mechanisms where valence electrons are shared in covalent bonds, but transferred (given/taken) in ionic bonds.