Chemistry Ch 6

Front 1

Periodic law

Back 1

When the elements are arranged in order of increasing atomic number, there is a periodic repetition of thier physical and chemical properties

Front 2

Metals

Back 2

One of a class of elements that are good conductors of heat and electric current; metals tend to be ductile, malleable, and shiny

Front 3

Nonmetals

Back 3

An element that tends to be a poor conductor of heat and electric current;nonmetals generally have properties opposite to those of metals

Front 4

Metalloid

Back 4

An element that tends to have properties that are similar to those of metals and nonmetals

Front 5

Alkali metals

Back 5

Any metal in Group 1A of the periodic table

Front 6

Akaline earth metals

Back 6

Any metal in Group 2A of the periodic table

Front 7

Halogens

Back 7

A nonmetal in Group 7A of the periodic table

Front 8

Noble gases

Back 8

An element in Group 7A of the periodic table; the s and p sublevels of the highest occupies energy level are filled

Front 9

Representative elements

Back 9

An element in an "A" group in the periodic table; as a group these elements display a wide range of phhysical and chemical propeties. In their atoms, the s and p sublevels of the highest occupies energy level are filled

Front 10

Transition metal

Back 10

One of the Group B elements in which the highest occupied s sublevel and a nearby d sublevel generally contain electrons

Front 11

Inner transition metal

Back 11

An element in the lanthanide or actinide series; the highest occupied s sublevel and nearby f sublevel of its atoms generally contain electrons; also called inner transition metals

Front 12

Atomic radius

Back 12

One-half the distance between the nuclei of two atoms of the same elements when the atoms are joined

Front 13

Ion

Back 13

An atom or group of atoms that has a positive or negative charge

Front 14

Cation

Back 14

An atom or group of atoms that has a positive charge

Front 15

Anion

Back 15

An atom or group of atoms that has a negative charge

Front 16

Ionization energy

Back 16

The energy required to remove an electron from an atom in its gaseous state

Front 17

Electronegativity

Back 17

The ability of an atom to attract electrons when the atom is in a compound

Front 18

How did chemists begin to organize the known chemists?

Back 18

Chemists used the properties of elements to sort them into groups

Front 19

How did Mendeleev organize his periodic table?

Back 19

Mendeleev arranged the elements in his periodic table in order of increasing atomic mass

Front 20

How is the modern periodic table organized?

Back 20

In the modern periodic table, elements are arranged in order of increasing atomic number

Front 21

What are three broad classes of elements?

Back 21

Three classes of elements are metals, nonmetals, and metalloids

Front 22

What type of information can be displayed in a periodic table?

Back 22

The periodic table displays the symbols and names of the elements, along with information about the structure of their atoms

Front 23

How can elements be classified based on their electron configurations?

Back 23

Elements can be sorted into noble gases, representative elements, transition metals, or inner transition metals based on their electron configurations

Front 24

What are the trends among elements for atomic size?

Back 24

In general, atomic size increases from top to bottom within a group and decreases from left to right across a period

Front 25

How do ions form?

Back 25

Positive and negative ions form when electrons are transferred between atoms

Front 26

What are the trends among the elements for first ionization energy, ionic size, and electronegativity?

Back 26

First ionization energy tends to decrease from top to bottom within a group and decrease from left to right across a period. Cations are always smaller than the atoms from which the form. Anions are always larger than the atoms from which they form. In general, electronegativity values decrease from top to bottom within a group. For representative elements, the values tend to increase from left to right across a period.

Front 27

What is the underlying cause of periodic trends?

Back 27

The trends that exist among these properties can be explained by variations in atomic structure