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Elements are

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Pure substances that cannot be separated into simpler substances by ordinary laboratory processes.

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Dmitri Mendeleev

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arranged the first 60 elements into groups.

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There are how many elements identified?

answer

118

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Elements arranged in

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the order of increasing atomic number.

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Vertical columns are called

answer

groups

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Groups contain elements with

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similar properties in vertical columns

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Horizontal rows of elements

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are periods

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Groups are number from

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1-18 or 1A-8A in earlier systems

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Periods are numbered from

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1-7

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Period 1 has how many elements

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2

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Period 2&3 have how many elements

answer

8

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Period 4&5 have how many elements

answer

18

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Period 6 has how many elements

answer

32

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A group's special name

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main group/Representative elements

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B Group's special name

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transition elements

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Alkali Metals are in Group

answer

1A

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Alkali Metals properties

answer

Soft, shiny metals
Good conductors of electricity and Heat
React vigorously with water
Form a white product when they react with oxygen
Hydrogen is not an alkali metal

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Alkaline Earth Metals properties

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Soft Shiny Metals
Conductors of Heat and Electricity
Reactive, but not as much as group 1 metals

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Halogens properties

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React with most elements

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Noble gases

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gases
nonreactive
Only a few compounds with other elements are known

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Alkali Metals Group

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1A or 1

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Alkaline Earth Metals Group

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2A or 2

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Halogens Group

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7A or 17

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Noble Gas Group

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8A or 18

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Metals are located

answer

on the left, except for hydrogen

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Nonmetals are located

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to the right

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Metalloids are located

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along the heavy zigzag line between the metals and nonmetals

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Properties of metals

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Metals are shiny solids except for mercury which is a liquid)
Malleable and ductile
They are good conductors of heat and electricity.
Melt at high temperatures
Have high densities

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Properties of nonmetals

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Nonmetals are dull brittle solids or gases at room temperatures.
Poor conductors
They are good insulators
Melt at low temperatures
Have low densities

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Properties of Metalloids

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Elements that have some properties similar metals and nonmetals
Are better conductors then nonmetals but not as good as metals
Are used as semiconductors and insulators

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All elements are made up of

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elements

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All atoms of the same element are

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identical

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Atoms are

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the smallest particle of an element that contain the characteristics of that element

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Dalton's Atomic theory-John Dalton

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Every element is made up of tiny particles called atoms

All atoms of a given element are identical. They are different from atoms of other elements.

Atoms of two or more different elements combine in a definite proportion to form compounds.

A chemical reaction involves changes in the arrangement or combination of atoms. (Atoms are neither created or destroyed)

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Electron Charge

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Negative

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Proton charge

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Positive Charge

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Protons and Neutrons are contained to

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A small region called the nucleus

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Neutrons charge

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neutral

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An atom consists

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of a nucleus that contains protons and neutrons

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Electrons are constantly moving in the large empty space around the nucleus

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called the electron cloud

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An atom of any element is electrically

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neutral the net charge of an atom is zero

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For a neutral atom

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protons=electrons in numbers

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The of which subatomic particle is negligible

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electron

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Where most of the mass in a atom

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the nucleus

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Chemist use atomic mass units

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to give masses of atoms and subatomic particles

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1amu=

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1/12 the mass of a C-12 atom with 6 protons and 6 neutrons

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Atomic Number is equal to the number

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of protons in an atom

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Atomic Number Appears

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above the the symbol of an element in the periodic table different from the nuclear symbol

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Mass Number

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is the sum of the number of protons and number of neutrons in the nucleus.

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Mass number=

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number of protons+number of neutrons

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Isotopes

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are atoms of the same element that have different mass numbers.
They have the same number of protons but different number of neutrons

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Nuclear Symbols

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Helpful when specifying isotopes.
Gives the Mass number in the upper left hand corner and the atomic number in the lower left corner.

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Atomic Mass is listed

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below the symbol of each element on the periodic table

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Atomic Mass gives the

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average of the atom

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Atom mass is

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a weighted average of masses of all isotopes based on their fractional natural abundances

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Electromagnetic Radiation

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Is energy that travels as waves through space
Moves at the speed of light in a vacuum
Is described in terms of wavelength and frequency

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Wavelength (lamda)

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is the distance between the top of a wave to the top of the next wave

is expressed in meters (m)

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Frequency (v,nu)

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is the number of waves that pass by each second

Is expressed in cycles per second also uses hertz

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Speed of light(c)=

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frequency x wavelength

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Electromagnetic Spectrum is

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a collection of all forms of electromagnetic radiation

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Visible light within

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wavelengths 700-400nm

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White light that passes through a prism

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is separated into all colors called a continuous spectrum.

gives the colors of a rainbow

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Atomic Spectrum

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consists of lines of different colors (line spectrum)

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What causes an atomic spectrum

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formed when light from a heated element passes through a prism.

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When an electron jumps to a higher energy level it

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absorbs energy

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An electron falls to a lower energy level by

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emitting energy

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Emitted radiation consists of small particles called

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photons

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The formula for the maximum number of electrons a energy level can hold

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2n^2

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the number of sublevels in an energy level is equal to

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the principal quantum number (n)

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Sub levels are designated with the letters

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s p d f

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Sublevels are also known as

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subshells

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maximum number of electrons in s

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2

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maximum number of electrons in p

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6

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maximum number of electrons in d

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10

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maximum number of electrons in f

answer

14

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S orbitals

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has one orbital that holds 2 electrons

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P orbitals

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have 3 orbitals and can hold 6 electrons

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d orbitals

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have 5 orbitals and can hold 10 electrons

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f orbitals

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have 7 orbitals and can hold 14 electrons

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Valence Electrons are

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the electrons in the highest (outermost) energy level

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Valence electrons in the electron configuration are the electrons in sublevels

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s and p with the highest n number

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All elements in the same group have

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the same number of valence electrons

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Number of valence electrons equal the

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group number if using the the 1a-8a numbering system

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Number of valence electrons equal

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group number - 10 if you are using the 1-18 numbering system

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Atomic radius is

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the distance from the nucleus to the valence electrons

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Atomic radius increases going down each group of Representative elements because

answer

the number of energy levels increases

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Atomic radius decreases going left to right across a period as

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more protons increase nuclear attraction for valence electrons

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Ionization energy is

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the energy it takes to remove a valence electron

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Metals have 1-3 valence electrons

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lower ionization energy

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Non metals have 5-7 valence electrons

answer

higher ionization energy

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Nobel Gases have complete octets (He has two valence electrons)

answer

have the highest ionization energies in each period

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