Chemistry Vocab List Chapter 3

Alkali metals

• all have 1 valence electron

• all have a common oxidation state (charge) of 1+

• all reactive with water

Alkaline earth metals

• each have two valence electrons

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Transition Metals

• all have partially filled in d-orbitals

• much less reactive than alkali metals

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Halogens

The 17th group of the periodic table, highly reactive nonmetals

Cation

An ion that has a positive charge (loses one electron)

Anion

A ion with a negative charge (gains one electron)

Metal

• regularly loses electrons to become a cation

• has a low effective nuclear charge relative to atomic radius

• has a low electron affinity

Nonmetal

• high effective nuclear charge relative to small radius size,

• highly negative electron affinity

Metalloid

• strong CLF and high effective nuclear charge

• highly negative electron affinity

Coulumb’s Law: formula and use

Formula: q1 times q2/r², used to calculate a valence electron’s attraction repulsion from another source

Effective nuclear charge

q2 in CLF, the values that we use in this equation are not exact values, the net positive charge experience by a electron in an atom

Ionization energy

the amount of energy gained by an atom when it loses an electron, always a positive value

Electron affinity

The amount of energy that is lost when an atom gains an electron, always a negative energy

Electronegativity

A numerical scale representing how much an atom attracts electrons to it

Atomic radius (size)

The distance from the nucleus of an atom to the edge of its electron cloud

Ion radius (size)

the distance from the center of an ion’s nucleus to the outermost edge of its electron cloud

Isoelectronic

two or more atoms, ions, or molecules that have the exact same number of electrons and the same electron configuration

Oxidation state

Charge of the ion