Elemental Properties and Types - AP Chemistry

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

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.

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.

Metallic compounds have unique properties due to their electron motility. In metals, electrons are able to move freely around and between atoms. In non-metals, electrons are more tightly bound to the nucleus due to increased nuclear positive charge and decreased atomic radius. The fluidity of electrons in metals allows them to conduct electric charge.

Metals are generally non-brittle. Metals are solids at room temperature and conduct electricity in the liquid phase, but they share these properties with a number of non-metal compounds as well.

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.

While many transition metals will lose an electron from the s shell before the d shell, many transition metals will lose only one electron from the s shell or none at all. The reason for this is that there is an enhanced stability when the transition metal's d shell is half filled, , so trasition metals will lose or not lose from the s shell in order to obtain a more stable electron configuration.

Electronegativity is defined as the tendency of an atom to attract an electron in a bond that it shares with another atom. Because oxygen wants to receive two elctrons, while both sodiums wish to lose one electron, oxygen has a higher electronegativity than sodium. Typically, electronegativity can be seen as increasing as you go to the top right of the periodic table. For example, fluorine has a higher electronegativity than nitrogen.