chemistry Module 5

ion

An atom or bonded group of atoms with a positive or negative charge

octet rule

States that atoms lose, gain, or share electrons in order to acquire the stable electron configuration of a noble gas

alkaline earth metal

Group 2 element in the modern periodic table and are highly reactive

electronegativity

Indicates the relative ability of an elements atoms to attract electrons in a chemical bond

group

the up and down (vertical) columns on a periodic table

Arranged in order of increasing atomic number; also called a family

halogen

A highly reactive group 17 element

inner transition metal

A type of group b element that is contained in the f-block of the periodic table and is characterized by a filled outermost orbital, and filled or partially filled 4f and 5f orbitals

ionization energy

The energy required to remove an electron from a gaseous atom; generally increases in moving from left-to-right across a period and decreases in moving down a group

metal

An element that is solid at room temperature, a good conductor of heat and electricity, and generally is shiny; most metals are ductile and malleable

metalloid

An element that has physical and chemical properties of both metals and nonmetals

noble gas

An extremely in reactive group 18 element

nonmetal

Elements that are generally gassed or dull, brittle solids that area poor conductors of heat and electricity

period

the horizontal rows on a periodic table

periodic law

States that when the elements are arranged by increasing atomic number, there is a periodic representation of their properties

representative element

Elements from groups 1, 2, and 13-18 in the modern periodic table, possessing a wide range of chemical and physical properties

transition element

Elements in groups 3-12 of the modern periodic table and are further divided into transition metals and inner transition metals

transition metal

An element in groups 3-12 that is contained in the d-block of the periodic table and, with some expectation, is characterized by a filled or partially filled d orbitals of energy level n-1

Antoine Lavoisier

Compiled a list f all known elements (23) in 1790. Discovered more and had 70 by 1870. No set organization.

John Newlands

1864 noted depiction in element properties every 8th element when arranged by increasing atomic mass. Called the law of octaves.

Dmitri Mendeleev

Worked with Lothse Meyer

Father of the periodic table

ordered by increasing atomic mass, noticed repetition

predicted properties of undiscovered elements

periodicity- the tendency to recur at regular intervals

Henry Moseley

discovered that atoms of each element contain a unique number of protons in there nuclei

the number of protons is equal to the atomic number

by arranging the elements in order of increasing atomic number instead of mass, it solved Tellurium

Properties of metals

luster, conduct heat, conduct electricity, high boiling point, malleable, ductile, solid, only mercury is in liquid state

location of metals on the periodic table

groups 1-13

properties of nonmetals

mostly gas

don’t conduct electricity or heat

brittle

lack luster

melting and boiling points are low

location of nonmetals on the periodic table

top right (staircase)

hydrogen, carbon, phosphorus, selenium, iodine, astatine

properties of metalloids

have properties of both metals and nonmetals

location of metalloids on the periodic table

between metals and nonmetals

boron, silicon, arsenic, tellurium, germanium, antimony

valence electrons of alkali metals

i valence electron (all in s¹)

valence electrons of alkali Earth metals

2 valence electrons (s²)

valence electrons of halogens

7 valence electrons (s2, p5)

valence electrons of noble gases

8 valence electrons, except helium (2 ve)

valence electrons of transition elements

often 2 ve-

valence electrons of inner transitions

2 ve-

alkali metal

group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements

Atomic radius

electron cloud surrounding nucleus

down/left

Ionic radius

up/right

Ionization energy

up/right

Electronegativity

up/right

location of alkali metals

group 1

valence electrons of alkali metals

1 ve

properties of alkali metals

basic, soft, highly reactive

location of alkaline earth metals

group 2

valence electrons of alkaline earth metals

2 ve

properties of alkaline earth metals

do not react with water, soft, good conductorsd

valence electrons of halogens

7 ve

properties of halogens

very reactive, salt-like

valence electrons of noble gasses

8 ve

properties of noble gasses

unreactive, bad conductors

valence electrons of transition elemnts

mostly 2

properties of transition elements

hard, luster, high melting/boiling ot, less predictable behavior

valence electrons of inner transitions

2?

properties of inner transitions

reactive, silvery

group 1 elements

alkalai metals

group 2 metals

alkaline Earth metals

group 17

halogens

group 1-2, 13-18

representative elemnts

groups 3-12

transition elements

two rows below the table

intertransition