Periodic Table Trends and Properties Review

Vocabulary practice flashcards covering periodic trends, atomic structure, orbital blocks, and element characteristics from chapter review problems 73 through 85.

Atomic Size in Bond Formation (Aspartame)

The principle that nonmetal atoms such as carbon, nitrogen, and oxygen decrease in effective radius when sharing electrons to form covalent chemical bonds, such as in aspartame.

Ion

An atom or a bonded group of atoms that has acquired a net positive or negative electrical charge.

Atomic Radius Measurement Limitation

The experimental constraint that an atom's radius cannot be measured directly because its surrounding electron cloud does not have a clearly defined or sharp outer boundary.

Boron ($B$)

The metalloid located in Period $2$ of the periodic table that is a constituent of chemical compounds utilized as water softeners.

Electronegativity (Cesium vs. Bromine)

A property comparison in which bromine, a halogen used in firefighting compounds, has a greater electronegativity than cesium, a Group $1$ element used in infrared lamps, because electronegativity increases across a period and decreases down a group.

Figure 22 (Periodic Table Blocks)

A visual mapping of the periodic table sections where Section A is the $s$-block, Section B is the $p$-block, Section C is the $d$-block, and Section D is the $f$-block, each grouping elements whose valence electrons occupy that specific orbital type.

Electronegativity Trends in Element Pairs

Periodic trends dictating that between $K$ and $As$, arsenic ($As$) is more electronegative; between $N$ and $Sb$, nitrogen ($N$) is more electronegative; and between $Sr$ and $Be$, beryllium ($Be$) is more electronegative.

Periodic Table Block Widths

The organizational feature where the $s$-block is two groups wide because an $s$ sublevel accommodates a maximum of $2$ electrons ($1$ orbital), the $p$-block is six groups wide because a $p$ sublevel accommodates up to $6$ electrons ($3$ orbitals), and the $d$-block is ten groups wide because a $d$ sublevel holds up to $10$ electrons ($5$ orbitals).

Mendeleev's Atomic Masses

Early atomic mass values that differ from modern values because historical measurements were less precise, unknown isotopes had not been accounted for, and modern atomic masses are weighted averages of naturally occurring isotopes.

Group 16 Atomic Radii Trend

An example of a group trend where atomic radius increases down a column due to the addition of principal energy levels, yielding the order of increasing radii: oxygen, sulfur, selenium, and tellurium ($O < S < Se < Te$).

Calcium ($Ca$)

An essential dietary mineral found in milk with the electron configuration $[\text{Ar}]4s^2$, positioned in Group $2$, Period $4$, and the $s$-block of the periodic table.

Period 1 p-Block Absence

The absence of $p$-block elements in the first period resulting from the fact that principal energy level $n = 1$ contains only an $s$ sublevel ($1s$), with $p$ sublevels only beginning at energy level $n = 2$.

Group 11 Jewelry Metals

Copper ($Cu$) and silver ($Ag$), the two transition metals in Group $11$ with the lowest atomic masses that are commonly utilized in jewelry making.

Ionization Energy (Platinum vs. Cobalt)

A comparison between cobalt, an element that imparts a bright blue color to pottery, and platinum, an element used in dental crowns, in which platinum possesses the larger ionization energy.