The Periodic Table - AP Chemistry

Atomic radius INCREASES DOWN and TO THE LEFT in the periodic table

Electronegativity increases across a period (going right) and decreases down a group \[not including noble gases\]. The element closest to the top right is Phosphorous

Non-metals are on the right side of the periodic table—past the metaloids and metals are on the left

As and Nb are the only combination that is a metal and non-metal

Rn is radon, a noble gas, which is not a metal. As a rule, elements to the left are metals, elements to the right are non-metals. The barrier would be the elements that are immideately to the right of the transition metals

Transition metals are found in the "middle" of the table

Na and Sr are metals

Cl and Po are non-metals

Metalloids are the groups of elements that separate the metals and non-metals; these form a "stair-case" on the periodic table

Transition metals have only partially filled valence bands. Thus, the electrons can move among the d orbitals, and this electron flow allows the transition metals to be good conductors of electricity.

The correct answer choice is an accurate explanation of effective nuclear charge. Since electrons are negatively charged, they are attracted to protons, which are positively charged. Protons are located in the nucleus of an atom.

The metals are found on the left side and the middle of the periodic table, and include the active metals, transition metals, and lanthanide and actinide series of elements. They easily give up electrons to form cations, since they have LOW ionization energies.

The number of neutorns is the only thing out of the answer choices that does not impact an element's atomic radius. Since neutrons have no charge, they do not impact the attractive forces between electrons and protons.

Selenium is on the right side of the periodic table, so it is not a metal or metalloid. It is not in column 7 or 8, so it is not a halogen or noble gas. Thus, it must be a nonmetal.

Electricity is produced and conducted by the movement of electrons, and thus the most important property that allows them to be used for wiring is their valence electrons that can move freely.

Hydrogen does not have enough space for 8 electrons, since it has only one s-subshell, which holds a maximum of 2 electrons.

This is the correct definition of ionization energy. By removing an electron from an atom, a cation is produced.

Metals are very large atoms that tend to lose electrons and become cations in solution. They will easily gain a positive charge, rather than a negative charge.

Metals typically have the following characteristics: they are malleable, ductile, and are excellent conductors for electricity. Metals are found on the left side of the periodic table.

Ionic bonds occur between metals and non-metals. The non-metal species are often halogens, very electronegative atoms which will completely take one of the non-metal's electrons. An ionic bond is not as much a bond as it is an association between positive and negatively charged atoms (ions). This association leads to the formation of rigid lattice structures of ionic compounds. Which makes them very stable, as seen by their high boiling points. When looking for ionic bonding, look for bonding between non-metals and metals, and atoms that are from opposite ends of the periodic table.

Atoms in the third period and above have d-orbitals that can hold up to 10 elecrons. This is what allows for atoms to exceed the octet rule.

B (boron) is one of the atoms known for making fewer than 4 covalent bonds, and therefore not filling its octet. C (carbon) always makes 4 bonds, while O (oxygen) and Cl (chloride) are also known for having full octets.

Rust forms when a substance is oxidized; thus iron cannot be a better oxidizing agent, because that would mean it would be more easily reduced. Aluminum and zinc are reactive, so that answer choice can be ruled out. Aluminum and zinc can form protective oxides by complexing the atom with oxygen.