M3 periodic table review

Atoms and the Periodic Table

u Chemists used the properties of elements to sort

the elements into groups.

u Mendeleev used increasing atomic mass to construct his

table.

u He knew some elements had similar chemical and

physical properties!

u He put each element on a card with its melting point

(MP) density, color, atomic mass and the # of bonds it
would form.

u He was able to predict undiscovered elements and their

properties after he arranged the cards by atomic mass!!

u Modern periodic table has elements arranged in

increasing atomic number (we needed to identify subatomic
particles before we could use atomic #)

When Mendeleev arranged his cards of elements

he noticed that the pattern was not quite right,
but when he moved a few cards over and left
spaces the pattern worked. He concluded that
the spaces were “yet undiscovered” elements.
He was able to predict the properties of these
elements!

6
C

Carbon
12.011

Atomic number.
Atomic symbol

Element name

Average atomic mass -

Review:
*To find the number of protons, see the atomic number.
*To find the number of electrons (see the atomic number)
*To find the number of neutrons, subtract the atomic number from the
atomic mass. Use whole number. 6 protons

6 neutrons

​12 atomic mass

Multiple Choice

How did Mendeleev arrange the elements?

• alphabetical 
• density
• melting point
• atomic mass

Multiple Choice

The number at the bottom of each square on the periodic table is the ...

• atomic number
• atomic mass
• chemical symbol
• element name

Multiple Choice

The number at the top of each square on the periodic table is the ...

• atomic number
• atomic mass
• Chemical Symbol
• Element Name

Multiple Choice

What is the chemical symbol for Lithium?

• H
• He
• Li
• N

V. How Do The Structures of the Atoms Differ?

A. Atomic Number - # of protons in the nucleus

1. Also tells the number of electrons in a neutral

atom

2. Each atom has a unique atomic number; never

changes

3. It identifies the atom
4. Usually the smallest number, always a whole #

B. Mass Number – sum of the protons + neutrons

1. Usually the biggest number, often a decimal

C. Ion – an atom or group of atoms that has lost or gained 1
or more electrons; therefore has a net (overall) charge
D. Isotope – atoms of the element with different numbers of
neutrons Ex: C-12 and C-14
E. Average Atomic Mass – weighed average mass of a
elements isotopes; why the mass is usually not a whole
number

uI: Organization of the Periodic Table

u A. Elements are arranged based upon atomic number

(# of protons). Usually the smallest of the 2 numbers

u Periodic Law – when elements are arranged the way there are

because of similarities in properties and it occurs in a regular
pattern.

u B. Period (series) – horizontal rows

u Number of protons and electrons increase by 1 as you move

across a period.

u C. Group (family) – vertical columns

u Elements in these groups have the same number of valence

electrons and have similar properties

Groups

Or

families

Periods

(when we write a sentence, we go ACROSS the paper and put a PERIOD at the end.)

Because the first
shell is full at 2 it
is at the end of
the period,

instead of
in the
second
group with
the other
elements
with 2
valence
electrons

Group 1

+1

Looses 1 -e

Group 2

+2

Looses 2 -e

Group

4

Group 5

-3

Gains 3 -e

Group 3

+3

Looses 3 -e

Group

6

Gains 2 -e

Group 7

-1

Gains 1 -e

Group

8

No charge

Transition metals

Variable charges

Less
(electrons) is
more (+) of a
charge

If you gain an
electron e- you
increase your
(-) charge

How Are Elements Classified

u Metals are usually shiny

solids that can be
stretched and shaped

They are ductile (put into

thin wire) and malleable(
hammered into sheets).

They are also good

conductors of heat and
electricity.

Most of the elements are

metals.

They are on the left side of

the periodic table

Form (+) ions

u Nonmetals (except H) are

found on the right side of
the chart. They may be
solid, liquid or gas…solid
ones are usually dull,brittle
(shatter if hit with a hamer)

Form (-) ions.
They are poor conductors of
electricity except for C

Alkali Metals - Group 1

u Soft, shiny metals

that react violently
with water and other
stuff.

u 1 valence electron in

this group=very
reactive. Will give up
an electron.

u Form 1+ ion

u Ex.: Sodium reacts

quickly with Cl to give
up an electron to it
and become NaCl,
salt.

u Must store in oil

Halogens - Group 7

u 7 valence electrons and

have a (-1) charge

u Very reactive; especially

with group 1

u Ex: Bromine (Br) – only

liquid nonmetal at room
temp

u Ex: Fluorine (Fl) – used in

toothpaste

u Ex: Chlorine (Cl) – used in

swimming pools

​Diatomic (bond together)
Boiling and melting points
decrease as you move
down.
Go from gas, liquid, solid as you move down.

Nobel gases - Group 8

u All gases. Different from most

elements, because they are very
unreactive.

u 8 valence electrons, so they won’t

react with any other elements.

u Also known as inert.

u Ex: Neon (Ne) - used in neon signs

(mixed with other elements gives
other colors).

u Ex: Helium (He) - is very light

(used in balloons).

u Ex: Argon (Ar) - used in light bulbs

to prevent it from burning up

Multiple Choice

The horizontal row on the periodic table is called a

• group
• family
• period
• atomic number

Multiple Choice

A vertical column is called...

• group
• tower
• period
• crew

Multiple Choice

Pure forms of these elements are stored in oil so they won't react with oxygen and water in the air.

• Alkali Metals
• Alkaline-earth metals
• Halogens
• Noble Gases

Multiple Choice

Most of the elements on the periodic table are classified as _____.

• Metals
• Nonmetals
• Metalloids
• Periods

Multiple Choice

How are elements on the periodic table arranged by?

• in alphabetic order
• simular physical & chemical properties
• their symbols
• Just simular physical properties

Multiple Choice

What element is will have the most similar physical and chemical properties to the element Bromine (Br)?

• Fluorine (F)
• Carbon (C)
• Krypton (Kr)
• Selenium (Se)

Multiple Choice

Elements that are arranged in __________ have the most similar physical and chemical properties to each other.

• periods
• groups

Multiple Choice

An atom is made up of protons, neutrons, and electrons.  Which is the smallest subatomic particle?

• Proton
• Neutron
• Electron
• Idontknowatron

Multiple Choice

The atomic number tells you what?

• number of electrons
• number of protons
• number of neutrons
• both electrons and protons in an atom.

Multiple Choice

Which group of the periodic table is composed of inert (not reactive)  gases?

• alkali metals
• alkaline earth metals
• halogens
• noble gases

Multiple Choice

Elements which are shiny, conduct electricity and heat are called

• metal
• nonmetal
• metalloid
• nonexistent

Multiple Choice

Which is an alkali metal?

• Magnesium
• Iron
• Sodium
• Europium

Multiple Choice

How many protons are in this element?

• 79
• 196
• 117
• Cannot be determined

Multiple Choice

How many electrons does potassium K contain? (click to see image)

• 19
• 39
• 20
• 40

Multiple Choice

How many neutrons are in a Gold atom?

• 79
• 196
• 118
• 275

Multiple Choice

What element is represented in this Bohr Model? 

• Carbon
• Hydrogen
• Aluminum
• Lithium

Multiple Choice

What's a valence electron?

• electrons in the second energy level
• electrons in the outermost energy level
• the atomic number
• electrons in the first level

Multiple Choice

The groups of the period table tell us:

• Number of electron shells
• Number or electrons
• Number of protons
• Number of valence electrons

Multiple Choice

The periods of the periodic table tell us:

• Number of valence electrons
• Number of electron shells
• Number of protons
• What's a period?

2
He

10
Ne

18
Ar

36
Kr

54
Xe

86
Rn

This group, the Noble gases (group18)
is usually very unreactive. This is
because they all have full valence
electron shells. Helium (He) has 2e in
the 1st shell (holds 2), Neon (Ne) has
2e in the lst shell, and 8e in the 2nd
shell (full).