College Prep Chemistry Unit 3 Periodic Table Review

Fill-in-the-blank practice flashcards covering Periodic Table trends, elemental families, electron configurations, cations/anions, and flame testing from Unit 3.

Atomic radius is defined as the __________ of an atom.

size

Electronegativity is defined as the attraction of an atom to a __________ pair of electrons.

shared

Ionization energy is defined as the energy needed to __________ an electron from an atom.

remove

Across a period, atomic radius decreases due to more __________ pulling energy levels closer to the center.

protons

Down a group, atomic radius increases due to the addition of more __________.

energy levels

Down a group, electronegativity and ionization energy decrease due to more __________ from having more energy levels.

shielding

Metal reactivity across a period decreases as ionization energy increases because electrons become __________ to lose.

harder

Metal reactivity down a group increases as ionization energy decreases because electrons become __________ to lose.

easier

Nonmetal reactivity across a period increases as __________ increases.

electronegativity

Noble gases do not have electronegativities because they do not __________ electrons with other atoms.

share

According to the graph, the element with atomic number 9 that has the greatest electronegativity is __________.

fluorine

A cation is formed by metals through the __________ of electrons, resulting in a positive charge.

loss

An anion is formed by nonmetals through the __________ of electrons, resulting in a negative charge.

gain

In the periodic table classification diagram, region 3 represents __________.

metalloids

According to the region map, the transition metal indicated is __________.

Ni

In region 6 of the periodic table, the period known as the rare earth metals is called the __________.

lanthanides

In region 6 of the periodic table, the period in which all elements are radioactive and mostly synthetic is called the __________.

actinides

Based on Element X's properties (solid, compound $XF_2$, configuration ending $s^2$, 3rd largest atom in the family), element X is __________.

strontium

Based on the periodic table families table, the predicted ion charge for the halogens family (Column 7A) is __________.

$$-1$$

The predicted ion charge for the alkali metals family (Column 1A) is __________.

$$+1$$

The predicted ion charge for the oxygen group family (Column 6A) is __________.

$$-2$$

The sublevels involved in valence electrons are always __________.

S and P

When an atom achieves the maximum of 8 valence electrons, it is referred to as a __________.

full octet

The full electron configuration for neutral magnesium is __________.

$$1s^2 2s^2 2p^6 3s^2$$

If a magnesium atom loses two electrons to form an ion, its new full electron configuration is __________.

$$1s^2 2s^2 2p^6$$

The valence electron configuration for chlorine is __________.

$$3s^2 3p^5$$

If a chlorine atom gains one electron to form an ion, its new full electron configuration is __________.

$$1s^2 2s^2 2p^6 3s^2 3p^6$$

During a flame test, electrons fall from high to low energy levels and release photons as light in a process called __________.

de-excitation

During a flame test, the group of elements that emit visible light (color) are __________.

metals

The term used to describe unreactive elements, such as the noble gases, is __________.

inert