Download Elements of the Periodic Table

Elements of the Periodic
Table
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Alkali Metals
-Found in group 1 of the periodic table.
-Very reactive metals that do not occur freely
in nature.
-Larger atomic radii
-Only 1 valence electron.
Properties of Alkali Metals
-Malleable and ductile
-Lower densities than other metals.
-Low melting and boiling points.
-Solid at room temperature.
-Good conductor of heat and electricity.
-Softer than most other metals.
-Can explode if exposed to water.
Alkali Metals-Examples
-Sodium(Na)
Forms useful compounds like table salt(NaCl), baking soda
(NaHCO3), soda ash(Na2CO3).
-Potassium(K)
Forms compound that can be used in fertilizers, glass,
soaps and detergents.
-Lithium(Li)
Used to make batteries, ceramics and lubricants.
Alkali Metals-Multiple Choice Qs
1. Which one of the following descriptions is
true of Alkali Metals?
A. High Densities
B. High Melting Points
C. Good Conductors
D. Not Reactive
Alkali Metals-Multiple Choice Qs
1. Which one of the following elements can be
used to make soap?
A. Lithium
B. Potassium
C. Sodium
D. Rubidium
Alkali Metals-Multiple Choice Qs
3. Alkali Metals have all of the following
properties EXCEPT
A. High Densities
B. Very Reactive
C. 1 Valence Electron
D. Soft
Alkaline Earth Metals These metals are a relatively soft shiny silverywhite color and they are in group 2A of the
periodic table. Alkaline earth metals are high in
reactivity, but not as high as group 1A. They
have stronger metallic bonding than group 1A
because there are two valence electrons. The six
metals in group 2A are Beryllium, Magnesium,
Calcium, Strontium, Barium, and Radium.
Description
Alkaline Earth Metals -
Representative
elements and uses
Barium (Ba): Used in paint and X-ray diagnostic work. Barium is also used for glassmaking and
making rubber. The carbonate in barium is used in rat poisoning.
Magnesium (Mg): Used for flares, pyrotechnics, and incendiary bombs. Magnesium is also useful in
aeroplane and missile construction. Another thing magnesium is used in is bricks and liners in furnaces.
Calcium (Ca): Calcium is essential for human nutrition, animal skeletons are made from the rigid
calcium and calcium helps to keep bones strong. Calcium helps build skeletal systems and maintains
muscle action. Calcium compounds are used in making lime, bricks, cement, glass, paint, paper, sugar,
and glazes.
Alkaline Earth Metals -
Properties
All Alkaline Earth Metals react with hydrogen to form metallic hydrides. Group
2A can also react with oxygen and halogens. All the elements in this group react
with water or steam except Beryllium. The average melting point for Alkaline
Earth metals is 831 degrees C and the average boiling point is 1661 degrees C.
They also have low densities, are not found freely in nature, and have an
oxidation number of +2.
Alkaline Earth Metals: Fun Facts!
BERYLLIUM occurs most commonly in beautiful minerals and gemstones such as emeralds, beryl
and aquamarine.
CALCIUM is the third most common metal on Earth.
STRONTIUM compounds are used in fireworks because of the red color it produces when burned.
MAGNESIUM is a key component of chlorophyll.
BERYLLIUM is toxic to humans and exposure to high concentrations can result in death.
RADIUM was once used in medicine to treat certain types of cancer and other conditions.
BARIUM is so reactive that it is stored under oil.
MAGNESIUM fires cannot be extinguished using carbon dioxide fire extinguishers.
Alkaline Earth Metals
Multiple Choice:
1) Which of the following is not an alkaline earth metal?
a. Barium b. Beryllium c. Titanium d. Radium
2) True of False: Group 2A has weaker metallic bonding than group 1A.
3) What Alkaline Earth Metal a component of bone?
a. Magnesium b. Barium c. Calcium
Group 13
Group 13 is usually referred to as the boron family.
The elements in group 13 belong to the p block on the periodic table and all have an
electron configuration ending in the p1 sub level.
Group 13 on the periodic table consists of Boron, Aluminium, Gallium, Indium, and
Thallium.
As you move down the group of elements the reactivity of them decreases.
Going down the elements they increase in atomic size, increase in density, increase in
ionic character, and decrease in polarity. The metallic characteristics also increase as
going down the group.
All of the elements in group 13 have a valence shell of 3 electrons.
Group 13-Properties
-In their physical properties aluminum, gallium, indium, and thallium are
metallic. Boron is the only element in the group that is a metalloid.
-The elements in group 13 have high boiling points, the highest being Boron at
about 4,000 degrees fahrenheit.
-The elements in group 13 are soft metals, with the exception of Boron,
which is a harder metalloid.
-Most of the elements in group 13 are metals, so tend to give up their 3
valence electrons, with the exception of Boron which tends to form covalent
bonds.
-The elements in group 13 are rare, with the exception of aluminum, which is
a very common metal
Group 13- Element Uses
Boron: Making enamel for covering steel, killing
cockroaches and aerospace travel.
Aluminum: Making auto parts, roofing and packaging food.
Gallium: Making transistors, converting electricity to light
and computer chips.
Indium: Coating bearings of cars, Making transistors and
making metal alloys.
Thallium: Infrared detectors, Making low melting glass and
pest killers.
Group 13 Multiple Choice
Which of the following elements is a metalloid?
a. Aluminum b. Thallium
c. Boron
d. Gallium
Which of these decreases while moving down group 13?
a. Ionic character b. polarity c. atomic size d. density
Which element is used for making computer chips and converting electricity to light?
a. Boron b. Thallium c. Aluminum d. Gallium
Group 14
-Consists of:
-Carbon (C) - non-metal
-Silicon (Si) - metalloid
-Germanium (Ge) - metalloid
-Tin (Sn) - metal
-Lead (Pb) - metal
-Each element in this group has four valence electrons. The electronic
configuration for each atom ends in p2.
-Ionization energies decrease the further you move down the group.
-The elements in this group become more and more metallic.
Group 14
Appearance: Carbon ranges from dull black color in the form of graphite, to transparent in the form
of diamond. Silicon and germanium are dull gray or black; tin and lead are a shiny gray color.
High melting points, ranging from 231.88 degrees (Sn) to over 3500 degrees (C)
All have densities greater than 1 g/cm3 (they would sink in water)
Carbon: 3.513 g/cm3
Silicon: 2.329 g/cm3
Germanium: 5.323 g/cm3
Tin: 7.130 g/cm3
Lead: 11.350 g/cm3
Group 14 Industrial Uses
- Carbon is used in almost everything in the industrial world (clothing,
dyes, fertilizers, fuels and new materials).
- Silicon is used mainly in the silicon chip, which has revolutionized
the computer industry.
- Germanium is used mostly in medicine. Researchers are interested
in using it as an alternative treatment for various cancers. But, it has
potentially deadly side effects.
- Tin is used to coat metals to prevent corrosion (like in tin cans).
- Lead has various industrial uses as well.
Group 14
-Carbon is found in the interior of stars; it is the fourth most abundant element with limitless
uses.
-Silicon is found in plant ashes and the human skeleton. It is an important ingredient in steel.
-Germanium is often used in fluorescent lamps and the glass in microscopes. It has a low
toxicity to mammals, but deadly for bacteria.
-Tin is often used in tin cans, providing a coating to steel to prevent corrosion.
-Lead is a poor conductor and resistant to corrosion. It is also highly poisonous.
Questions for Group 14
1. Which of the following elements is a non-metal?
a. Tin
b. Silicon c. Germanium
d. Carbon
2. How many valence electrons are in the outer shell of each element?
a. 2
b. 0
c. 4
d. 14
3. Which element is found in plant ashes?
a. Silicon
b. Lead
c. Carbon
d. Tin
Group 15: The Nitrogen Family
Group 15 in the periodic table is called pnictogen. It is also known as the
nitrogen family. It includes the elements nitrogen(N), phosphorus(P), arsenic
(As), antimony(Sb), and bismuth(Bi). All of the elements in this group have 5
electrons in their outer shell. All of these elements are solid at room
temperature except for nitrogen (which is a gas).
Metals: Bismuth
Nonmetals: Nitrogen, Phosphorus
Metalloids: Arsenic, Antimony
Group 15: The Nitrogen Family
Physical Properties:
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Nitrogen is a colorless, odorless gas.
The other elements are usually solids.
Melting and boiling points vary with Nitrogen freezing at -210*C and
liquefying at 200*C and Bismuth boiling at 1560*C.
Chemical Properties:
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Nitrogen is very unreactive.
Phosphorus reacts with different elements to form phosphides, sulfides,
halides, and oxides.
Nitric acid is very reactive.
All the elements of this group have 5 electrons in their outer energy
levels.
Group 15: The Nitrogen Family
Representative elements & uses:
Nitrogen (N) - used in ammonia which is used for fertilizer production and to
make nitric acid, used by the electronic industry
Phosphorus (P) - used to make safety matches, pyrotechnics, smoke bombs,
tracer bullets etc., fertilizers, used in the production of special glasses
Arsenic (As) - used for bronzing and pyrotechnics
Antimony(Sb) - used to increase the mechanical strength of lead, used to
make batteries, type metal, small arms, and tracer bullets
Bismuth (Bi) - used to make malleable irons, used for fire detection
Multiple Choice Questions
1) How many valence electrons do the elements of group 15 have?
a. 7
b.1
c. 5
2) What is group 15 known as?
a. the nitrogen family
b. the proud family
c. the atoms family
3) Which of the elements is not solid at room temperature?
a. antimony
b. arsenic
c. nitrogen
Group 16
● Group 16 of the Periodic table is also
called Chalcogens or the Oxygen
Family
● Oxygen & sulfur are nonmetals
● Selenium, tellurium, and polonium
are metalloids
Properties of Group 16 Elements
● They have 6 electrons in their outermost shell.
● High boiling points except oxygen
● P block elements (s2 p4)
● All have high densities except oxygen
Group 16 Element Uses
Oxygen Sulfur Selenium Tellurium Polonium
● Sulfur can be used in gunpowder
● Polonium is a radioactive metal, and therefore has no common
uses
Group 16 Multiple Choice Questions
1.) Which element in Group 16 is the only one with a low boiling point and a low density?
a) Polonium
b) sulfur
c) oxygen
2.) How many valence electrons does each element in Group 16 have?
a) 6
b) 8
c) 16
3.) Which of the following is not an element in Group 16?
a) Selenium
b) Barium
c) Tellurium
Halogens
-The word halogens means salt-formers.
-They are non-metal elements
-They exist in solids, liquids and gases in room
temperature. (Fluorine and chlorine are gases, bromine is
solid and iodine is liquid.)
-They are one electron away from having a full valence
shell.
-They are poisonous.
Halogen - Properties
-Most reactive of the elements
-Poor conductors of heat and electricity
-They are diatomic molecules (compounds are formed
by two atoms)
-All have 7 electrons in their outer shell
-The melting points and boiling points start low and
as you go down the group they increase to a high
melting and boiling point.
-Fluorine is colorless, chlorine is pale green, bromine
is dark red/brown and iodine is very dark violet.
Halogen- Uses
Iodine - Used as a pharmaceutical, printing inks,
and as a catalyst in animal food
Fluorine - Used in the manufacture of Teflon
which is used in pots, pans, and refrigerators
Bromine - Used to purify water, as pesticides,
leaded fuel for cars, and manufacture of
medicines
Chlorine - Used to make chloroform, disinfect
pools, and make products like paper and
petroleum products
Halogens - Fun Facts
-None of the halogens can be
found in nature in their
elemental form.
-They are found in salts of the
halide ion in oceans and lakes of
high salt content.
-Fluorine is so reactive it causes
most metals to burst into
flames.
Halogen - Multiple Choice
1.Are Halogens very reactive?
a. Yes
b. Only a little bit
3. Where can their ions be found?
c. No
a. oceans & lakes of high salt
content
2. What does the word “Halogen”
mean?
b. trees
a. salt-former
c. can’t be found on earth
b. pizza
d. the air
c. non-reactive
d. fire
Noble Gases
The noble gasses are non-metals, located in the furthest
group to the right side of the Periodic Table (18). All of the
noble gases are colorless, odorless and in a gaseous state at
room temperature, and being gases, they have extremely low
boiling points. They also have high ionization energies and low
electronegativity. The Noble Gases are relatively non-reactive
because they have eight valence electrons. With a full valence
shell, elements tend to be more stable.
Noble gas elements
One very useful noble gas is neon. Although neon is colorless, when one runs an electric
charge through a tube of the substance it glows a reddish orange color. These true neon lights are
mainly used for advertising signs when a business wants to catch the eye of potential customers.
Neon can also be used to make high voltage indicators, lightning arresters and as an extremely
powerful refrigerant.On top of this neon is a rare non-toxic gas that appears in 18 parts per million
of air.
Xenon gives off a bright white light that is often used in commercial lighting applications
including spotlights and movie projectors. Xenon can be used as a powerful anesthetic when inhaled
but its high cost has kept it from becoming commercially viable allowing it to compete with nitrous
oxide. It is 44% more potent as an anesthetic than nitrous oxide.
A very common noble gas, as a matter of fact the second most abundant element in the
universe is Helium. Helium represents about 24% of the elemental mass (remember, there are over
one hundred elements..) It is the second lightest element, it ONLY exist as a
gas except for in extreme conditions and is seen as a yellow line on the electromagnetic spectrum.
Noble gas Questions
1. Noble gases are very reactive.
A. True
B. False
2. Neon can be used as a _______.
A. Refrigerant B. Semi-Conductor C.Heat Source
3. Noble gases are _______.
A. Metals B. Metalloids C.Non-metals
Description of Transition Metals
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The 38 elements in groups 3
through 12 of the periodic table
are called “transition metals.”
In the past, all of the elements in
the d-block of the Periodic Table
of Elements were referred to as
transition metals. Now, a
transition metal is an element
whose atom has an incomplete dsub shell.
All these elements are metals.
Representative Elements and Uses
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Three noteworthy transition metals are iron, cobalt and nickel. These are the only
elements known to produce a magnetic field.
The most abundant transition metals are Iron and Titanium.
■ Iron is the cheapest available metal, mostly used to manufacture steel.
Ordinary carbon steel is an alloy of carbon with iron.
■ Titanium is important as an alloying agent with many metals. These
alloys are principally used in aircrafts and missiles as they have low
density but can withstand high amounts of heat.
Properties of Transition Metals
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High melting points
High boiling points
High electrical conductivity
Low ionization energies
Positive oxidation states
Malleable
Other Information
● The f-block lanthanide and actinide series are also
considered transition metals and are called "inner
transition metals"
● The transition elements have positively charged forms
or stable oxidation states which allow them to form
many different ionic and partially-ionic compounds.
● Transition metal valence electrons are present in more
than one shell.
Multiple Choice Questions for Transition Metals
1) Which sublevels are partially filled in Transition Metals?
A) f
B) s+p
C) d+f
2) What are the f-block elements occasionally called?
A) inner transition elements
B) outer transition elements
C) f-block transition elements
3) One key characteristic of the Transition Metals is
A) they are colorless
B) they are unreactive
C) their valence electrons are found in more than one shell