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M-2 Elements of Periodic
Table
Alkali Metals
Alkali metals are the first group in the periodic
table. They are all shiny, soft metals. They are
highly reactive at room temperature and standard
pressure, and readily lose their valence electrons.
Alkali
Metals!
More About Alkali Metals!
Hydrogen is in the not classified as
an Alkali metal because it has
several different properties, but when
it is considered an alkali metal it is
because of its atomic properties and
not because of its chemical
properties.
Na- Sodium Chloride is
also known as salt. Also
sodium can be used for
cleaning.
Li- Lithium Batteries,
some ceramics and
glasses.
Cs-Cesium is used in
photoelectric cells and vacuum
tubes.
Rb- Rubidium can be used
for space vehicles, also
making special gases.
Fr- Francium has
no uses.
K- Potassium is mostly used for
health benefits, it helps fight against
many different things, such as high
blood pressure.
Three Questions for You!
1. What are alkali metals?
2. Why is hydrogen not
considered an alkali metal?
3. What are three alkali
metals and what are they
used for?
Alkaline Earth Metals...
-Be: Beryllium (4); Used to make hand tools.
-Mg; Magnesium (12); Used in pyrotechnics and flares.
-Ca; Calcium (20); Used in nutrient supplements for strong bones.
-Sr; Strontium (38); Used in red fireworks.
-Ba; Barium (56); Used in paint and glass making.
-Ra; Radium (88); Used in forms of cancer therapy.
Alkaline Earth Metals
Description: Alkaline earth metals are elements found in the second group of
the periodic table. These elements are metals and therefore somewhat
reactive. They are metals with a shiny, silvery-white colour. These elements are
found in the Earth’s crust.
Properties: of Alkaline Earth Metals
* 2 valence electrons
* Low electron affinities
* Usually lose 2 electrons to form divalent cations.
Questions
1.- In what Group are Alkaline Earth metals
found?
a. Group 1
b. Group 2
c. Group 3
d. Group 18
2.- How many valence electrons do Alkaline
Earth metals have?
a. 4
b. 3
c. 1
d. 2
3.- Where do Alkaline Earth metals come from?
a. space
b. air
c. from human making
d. Earth’s crust
4.- Why are Alkaline Earth metals less reactive than
Alkaline Earth metals?
a. because they are not metals
b. because they come from outer space
c. because they have 2 valence electrons instead of
1.
d. because they melt easier
Group 13
Properties
Boron is a non-metallic gray powder, but all of the other elements in group
13 are soft, silvery metals.
All of the elements have high melting points and high densities.
Most of the elements are relatively reactive with the exception of Boron.
All of the metals are good conductors and Boron is a good insulator.
Group 13
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Boron (B), Aluminum (Al), Gallium (Ga), Indium (In), Thallium (Tl)
The elements in group 13 all have three valence electrons.
They become more reactive as their atomic mass increases.
All of group 13’s elements commonly form a covalent bond with three
oxygen atoms.
They are also known to form compounds with elements in the Halogen
group.
Uses for group 13 elements include fiberglass, ceramics, coatings,
components in LED lights, components in electrical devices, and dental
purposes.
Thallium is banned in the United States because of its toxicity.
Group 13
1. Which element in this group is the metalloid?
a) Gallium
b) Boron
c) Thallium
2. Which block is this group located in?
a) D
b) S
c) P
3. Which element has the electron configuration of 1s2 2s2 2p6 3s2 3p1?
a) Gallium b) Aluminum c) Indium
Group 14
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Group 14 contains Carbon, Silicon, Germanium, Tin, and Lead.
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Elements in this group have 4 valence electrons.
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Carbon is a metal, Silicon and Germanium are metalloids, and Tin
and Lead are nonmetals.
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Elements in Group 14 are solid at room temperature.
Property of Group 14
Physical Properties:
Chemical Properties:
Carbon can’t conduct electricity.
Carbon has a unique ability of catenation to
form stable compounds.
Silicon is a semi-conductor.
Silicon is unreactive chemically. It is not attacked
by aqueous acids, but does react with
concentrated alkalis.
Tin and Lead, similar to other common metals,
are good conductors of electricity.
Germanium is similar to Silicon.
Tin and Lead are quite easily oxidized.
The Importance of Carbon
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Group 14 is also referred to as the Carbon Family because Carbon is
necessary to live.
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Carbon is found in basically every molecule of every living thing.
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Roughly 18% of body mass is Carbon.
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Carbon is found in the sun, stars, comets, and almost everything else.
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Its boiling point is 3825˚ C
Great Group 14
Industrial Information
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Carbon is used extensively in almost all areas of modern civilization; clothing, dyes,
fertilisers, agrochemicals, fuels and new materials.
Silicon also contributes to new technology in the silicon chip, which has
revolutionised the computer and high-tech industries.
Germanium, like silicon, is a semi-conductor used in similar devices, but it is less
widely used.
Tin is used as a coating for other metals to prevent corrosion, such as in tin cans.
Lead is used in great quantities in storage batteries. It is also used in cable covering,
for roofing in buildings and for radiation shielding. It was used in the manufacture of
tetraethyl lead, an anti-knocking compound added to petrol, but this was shown to
be an environmental hazard.
Questions About Group 14
1. How many valence electrons are in elements of Group 14?
a. 6
b.4
c.9
d.1
2. What percentage of body mass is Carbon?
a.13% b.19% c.2%
d.18%
3. What element is NOT found in Group 14?
a. Nitrogen b.Silicon
c.Carbon
d.Lead
Group 15
By: Sydnie Picard and Josh Pickus
Group 15
The elements in group 15 are apart of the Nitrogen
family. As the elements in group 15 descend, their
metal characteristics become more prominent. Within
this group is, nitrogen (N), phosphorus (P), arsenic
(As), antimony (Sb), and bismuth (B). Bismuth is a
metal, arsenic and antimony are the metalloids, and
nitrogen and phosphorus are non-metals.
Properties of Group 15
Element/
symbol
Atomic Number
Mass
Electron
Configuration
Physical Forms
Nitrogen (N)
7
14.01
1s22s22p3
Colorless Gas
Phosphorus (P)
15
30.97
[Ne] 3s23p3
White Solid/
Red Solid
Arsenic (As)
33
74.92
[Ar] 3d104s24p3
Yellow Solid/
Gray Solid
Antimony (Sb)
51
121.76
[Kr] 4d105s25p3
Yellow Solid/
Silver-White
Metallic Solid
Bismuth (Bi)
83
208.98
[Xe]
4f145d106s26p3
Pink-White
Metallic Solid
Uses
Nitrogen- laughing gas, smog,
neurotransmitters, and rocket fuel.
Phosphorus- baking powders, cheese, instant
cereals, curing ham, and soft drinks.
Arsenic- weed killers, insecticides, and
alloys.
Antimony- batteries, and it helps make
alloys.
Bismuth- cosmetic products and medicine.
Questions:
1. What is the electron configuration of
Arsenic?
a. [As]3d104s24p3 b. [Ar]3d104s24p3 c. 1s22s22p63s2
2. Nitrogen
and Phosphorusb.are
metals.
False
a. True
3. What is the most common physical form of
Nitrogen?
a. metallic solid
c. colorless gas
b. clear liquid
Group 16 - Chalcogens
Chalcogens are
contained in group 16
on the Periodic table.
They are also referred
to as the “Oxygen
Family”.
The Elements
Properties
Oxygen - Nonmetal - Gas
combustible, reactive,
Sulfur - Nonmetal - Solid
combustible, reactive, reductive,
Selenium - Nonmetal - Solid
Tellurium - Metalloid Solid
combustible, reactive,
can show properties of both metals
and nonmetals
conducts heat and energy well,
radioactive, volatile.
Uses
Oxygen - breathing apparati, rocket
fuel, blow torches
Sulfur - battery fuel, bleach dried
fruit, paper products
Selenium - rectifiers, stainless steel,
shampoo
Tellurium - tinted glass, lubricants,
ceramics
Polonium - heat source in space
equipment, nuclear weapons
Other Information
● All are found in
copper ore.
● The elements have
6 valence
electrons.
● They can generate
acid.
● They have the
ability to catenate,
meaning, they
bond with atoms of
the same element.
Questions
1. Which of the following is NOT a member of the
Chalcogen family?
a. Tellurium
b. Potassium
c. Sulfur
2. Which of the following is a use of Selenium?
a. Breathing Apparati b. nuclear weapons c. shampoo
3. How many valence electrons does each element have?
Halogens- Nonmetals
Description: Halogens are the five toxic, non-metallic elements that can be found in group 17 of
the periodic table. Compounds that contain halogens are called salts since halogen itself means
“salt former”
Physical Properties:
•Have seven valence electron
•Exist in all three states of matter: solid, liquid and gas
•Are diatomic when kept under room temperature
•No halogen is completely colorless
•In solid forms, all halogens will have brittle texture
Chemical Properties:
•Gain electrons very fast
•Are poor conductors of heat and electricity
•Have low melting and boiling points
•Form very strong acidic compounds with hydrogen called halides
•Highly reactive especially with alkali metals
•Very high electronegative
Halogens- The Elements
Fluorine (F): used in refrigerants and detergents, produces sulfur hexafluoride
in electrical industry.
Chlorine (Cl): used as bleach, to treat waste water and sewage, and
purification of drinking water and swimming pools.
Bromine (Br): used in coal power plants to reduce mercury levels, disinfect
water, fumigants and flame proofing agents.
Iodine (I): used as sterilizing agents, treats allergies, tests for starch, used in
photography and xrays.
Astatine (At): used in the treatment of cancer, and a radioactive tracer.
Quiz Yourself
1. Where are halogens found on the
periodic table?
2. How many valence electrons does a
halogen have?
a. Left
a. 2
b. Right
b. 6
c. Top
c. 7
d. Bottom
d. 8
3. Which of these is NOT a property of
Halogens?
a. Reactive
b. Diatomic
c. High electronegativities
d. Nonmetallic
e. All are properties of Halogens
Fun Facts about Halogens!!!
Bromine liquid evaporates easily at room
temperatures emitting an orange vapor.
Halogen comes from Greek words “hals”
meaning “salt” and “gen” meaning “to make”.
Noble Gases
Helium, Neon, Argon, Krypton, Xenon, Radon
Abbey Dowling and Jacob Bennert
What are Noble Gases?
● The Noble Gases consist of Helium (He), Neon (Ne), Argon
(Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn).
● Radon is radioactive.
● Each Noble Gas has a full shell of outer valence electrons.
● They aren’t very chemically reactive.
● They are non-metals (obviously).
● Neon, Argon, Krypton, and Xenon are all obtained from the
air.
● Helium is obtained from natural gas.
● Radon is the product of decay from Uranium.
What are the Properties of Noble
Gases?
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Helium’s melting and boiling points are lower than those of any
other known substance and is the only element that cannot be
solidified by cooling under standard conditions.
All of the Noble Gases have very low melting and boiling points, and
are all very close together, meaning that they are liquids over only a
small range of temperatures.
Under standard conditions they are all odorless, tasteless, and
colorless.
How can you use a Noble Gas?
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Helium (He)-Used in filling balloons, a cooling medium for nuclear
reactors, a mixture of 80% helium and 20% oxygen is used as an
artificial atmosphere for divers and others working under pressure.
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Argon (Ar)- used to fill incandescent and fluorescent light bulbs, and
creates an inert atmosphere for processes that require shielding
from other atmospheric gases.
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Xenon (Xe)- Used in photography when instant intense light is
required. Also used in electron tubes, stroboscopic lights and
bactericidal lamps.
What have you learned?
1.What are the Noble Gases?
a. Helium, Neon, Argon, Krypton, Xenon, Radon
b. Helium, Argon, Neon, Xenon, Hydrogen, Radon
c. Helium, Neon, Argon, Iodine, Xenon, Radon
2. What do Noble Gases taste like?
a. Chocolate
b. You can’t taste them
c. Chicken
d. Water
3. Which Noble Gases are obtained from the air?
a. All of them
b. Helium, Krypton, Hydrogen, Xenon
c. All but Helium and Radon
Transition Metals
By Kevin Smith, Emily Richards, Conor
Purvis
Transition Metals
● Transition Metals are the elements located in groups 3 through
12, or the d-block, on the periodic table.
● These 38 elements have partially filled d or f sublevels in any
common oxidation state
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Unlike other elements on the periodic table, the valence
electrons for transition metals are found in more than one shell.
● The elements found in the transition metals are all metals.
Properties
The transition metals are elements that have a partially filled d
sublevel in the outer valence shell. Transition metals are much alike
regular metals. Some properties are:
● They are very hard,
● Have a high melting point,
● They also have several oxidation states,
● And they usually form colored compounds.
Facts about Transition Metals
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Three transition metals, Iron, Nickel, and Cobalt are the only elements
that can produce a magnetic field.
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Chemist use a “d electron count” instead of valence electron to
describe transition metals.
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Transition metals are often used as catalyst in various reactions
because of their unique qualities
Examples of Transition Metals
Iron (Fe) Z=26
Silver (Ag) Z=47
Yttrium (Y) Z=71
Hafnium (Hf) Z=72
Iron is one of the cheapest and
most common metals on Earth. It
is used to make steel which is
commonly use in Architecture.
Platinum (Pt) Z=78
Cobalt (Co) Z=27
Cobalt is used in electroplating. It
gives objects an attractive surface and
resist oxidation. It is also used to
make alloys for jet engines and gas
turbines, types of stainless steel and
magnetic steels.
Dubnium (Db) Z=105
Nickel (Ni) Z=28
Nickel can be used as a
protective coating. Nickel can
also be used as a catalyst for the
hydrogenation of vegetable oil.
You can give glass a green color
by using Nickel.
Questions
1. Transition metals have a partially filled __ sublevel in their outer shell.
a) s
b) p
c) d
d)f
2. The transition metals are located in what groups?
a) 1-7
b) 3-12
c) 9-18
d) 13-15
3. Transition metals have __ elements?
a) 28
b) 37
c) 40
d) 38
Inner Transition Metal
By Julia Rowlett, Maggie Connellan, and Libby Vaughan
Inner Transition Metal Description
The Inner Transition Metals are the elements
57-70 (lanthanides) and 89-103 (actinides).
These metals are generally found below the
Periodic Table. The Inner Transition Metals are
also known as the f-block. There are two
different types of Inner transition Metals, the
lanthanides and the actinides. The lanthanides
are are found naturally on Earth and are know as
the “rare Earth metals”. The actinides are not
found naturally, and tend to be very reactive.
Inner Transition Metal Properties
Lanthanides
(“Rare Earth Metals”)
metals; silvery-white
color; relatively soft;
high melting points and
boiling points; very
reactive; paramagnetic;
powerful magnetics
Actinides
metals; silvery color;
soft; radioactive; high
density; pyrophoric;
combine directly with
most nonmetals; tarnish
in air; paramagnetic;
highly unstable; give up
electrons easily
Inner Transition Metal Uses
● All actinide elements are radioactive, and some are
used for nuclear power. For example, uranium and
plutonium isotopes are used in nuclear weaponry.
● Some lanthanide metals (neodymium, gadolinium,
and samarium) are used to create powerful magnets
because of their magnetic properties. Gadolinium is
used at hospitals in MRI and X-ray machines.
Inner Transition Metal Questions
1. Which inner transition metals are radioactive?
Lanthanides/Actinides
2. Which element is used in hospital machinery because
of its magnetic properties?
Plutonium/Gadolinium/Lanthanum
3. The inner Transition Metals are located in which
“block” on the periodic table?
s-block, p-block, d-block, or f-block