Vocabulary Periodicity

 

1 affinity An attractive force between substances or particles that causes them to enter into and remain in chemical combination
2

alkali metals

The Group 1 elements, lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr) react with cold water for form strongly alkaline hydroxide solutions, and are referred to as "alkali metals". Hydrogen is not considered an alkali metal, despite its position on some periodic tables.

3

alkaline-earth metals

The Group 2 elements, beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra) form alkaline oxides and hydroxides and are called "alkaline earth metals".

4

atomic radius

One half the distance between nuclei of atoms of the same element, when the atoms are bound by a single covalent bond or are in a metallic crystal. The radius of atoms obtained from covalent bond lengths is called the covalent radius; the radius from interatomic distances in metallic crystals is called the metallic radius.

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Average atomic mass

Most elements occur in nature as a mixture of isotopes (i.e. populations of atoms with different numbers of neutrons, and therefore, mass). We can calculate the average atomic mass of an element by knowing the relative abundance of each isotope, as well as the mass of each isotope.  The average atomic mass of each element (in amu) is also referred to as its atomic weight. Values for the atomic weights of each of the elements are commonly listed in periodic tables.

6

Avogadro’s number

The number of particles in one mole, equal to 6.02214199 × 1023 mol-1 (± 0.00000047 mol-1)  Also called Avogadro constant.  (NA, L)

7

chemical properties-

Measurement of a chemical property involves a chemical change. For example, determining the flammability of gasoline involves burning it, producing carbon dioxide and water.

8 diatomic element Consisting of two atoms : having two atoms in the molecule.  Naturally occurring diatomic elements are H2, N2, O2, F2, Cl2, Br2, and I2.
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electronegativity

Electronegativity is a measure of the attraction an atom has for bonding electrons. Bonds between atoms with different electronegativities are polar, with the bonding electrons spending more time on average around the atom with higher electronegativity.

10

element

An element is a substance composed of atoms with identical atomic number. The older definition of element (an element is a pure substance that can't be decomposed chemically) was made obsolete by the discovery of isotopes.

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families

A group of elements with similar chemical properties.

12

gram/mole conversions

The formula weight (or molecular weight or molar mass) of a compound tells you how many grams are in one mole of the compound. This gives you a way to convert from grams to moles or moles to grams.

13 Groups Columns in the periodic table are called groups. For example, all of the elements in the second column are referred to as 'second group elements'.
14

halogens

An element of group VIIA (a. k. a. Group 18). The name means "salt former"; halogens react with metals to form binary ionic compounds. Fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At) are known at this time.

15 Inert Gas see Noble Gas
16

ion size/ion radius relation

A cation is smaller than it’s neutral atom because it has lost electrons. An anion is larger than the neutral atom because it has gained an electron.

17

ionization

The formation of or separation into ions by heat, electrical discharge, radiation, or chemical reaction.  The state of being ionized.

18

ionization energy

The energy needed to remove an electron from a gaseous atom or ion. It is also called (IE,IP) ionization potential.

19

lanthanides

Elements 57-70 are called lanthanides. Electrons added during the Aufbau construction of lanthanide atoms go into the 4f subshell.

20

mass number (M,A)

The total number of protons and neutrons in an atom or ion. In nuclide symbols the mass number is given as a leading superscript. In isotope names (e. g. carbon-14, sodium-23) the mass number is the number following the element name.

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Mendeleev

Russian chemist who first devised and published the periodic table of the elements (1869).

22

metal or  metallic

A metal is a substance that conducts heat and electricity, is shiny and reflects many colors of light, and can be hammered into sheets or drawn into wire. Metals lose electrons easily to form cations. About 80% of the known chemical elements are metals

23

metalloid / semi-metal

An element with both metallic and nonmetallic properties. Examples are silicon, arsenic, and germanium.

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molar mass

The mass of one mole of a material. For example, the molar mass of H2O is 18.015 g (obtained by adding twice the molar mass of hydrogen to the molar mass of oxygen).

25

noble gases

Any of the elements in Group 18 of the periodic table, including helium, neon, argon, krypton, xenon, and radon, which are monatomic and with limited exceptions chemically inert. Also called inert gas.

26

noble-gas configuration

The noble gases are chemically inert - that is that they do not react. Examination of their electronic configurations reveals that, except for helium, they all have the filled s and p orbitals. This observation suggests that we can attribute their lack of chemical reactivity to this filled s and p electronic configuration. 

Noble Gas

Electronic congifuration

He 

1s2 

Ne

[He]2s2 2p6

Ar 

[Ne]3s2 3p6

Kr

[Ar]3d10 4s2 4p6

Xe 

[Kr]4d10 5s2 5p6

Rn

[Xe]4f14 5d10 6s2 6p67

 

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nonmetal

A nonmetal is a substance that conducts heat and electricity poorly, is brittle or waxy or gaseous, and cannot be hammered into sheets or drawn into wire. Nonmetals gain electrons easily to form anions. About 20% of the known chemical elements are nonmetals.

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Periods

Rows in the periodic table are called periods. For example, all of the elements in the second row are referred to as 'second period elements'.

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period trends

A regular variation in element properties with increasing atomic number that is ultimately due to regular variations in atomic structure.

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periodic law

The periodic law states that physical and chemical properties of the elements recur in a regular way when the elements are arranged in order of increasing atomic number.

31

periodic table

An arrangement of the elements according to increasing atomic number that shows relationships between element properties.

32

periodicity

The quality or state of being periodic; recurrence at regular intervals.  The repetition of similar properties in chemical elements, as indicated by their positioning in the periodic table.

33 semi-metal - see metalloid
34 s, p, d, and f   blocks

s block - groups 1and 2  ; p block - groups 13 through 18 ; d block groups 3 through 12 ;

f  block - the actinide and lanthanide series

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transition elements

An element with an incomplete d subshell. Elements which have common cations with incomplete d subshells are also considered transition metals. Elements with incomplete f subshells are sometimes called "inner transition elements".

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valence electrons

Electrons that can be actively involved in chemical change; usually electrons in the shell with the highest value of n. For example, sodium's ground state electron configuration is 1s2 2s2 2p6 3s1; the 3s electron is the only valence electron in the atom. Germanium (Ge) has the ground state electron configuration 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p2; the 4s and 4p electrons are the valence electrons.

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valence shell

The shell corresponding to the highest value of principal quantum number in the atom. The valence electrons in this shell are on average farther from the nucleus than other electrons; they are often directly involved in chemical reaction.