review when looking at atoms, what three numbers are the same? how do you find the number of...

Review• When looking at atoms, what three

numbers are the same?• How do you find the number of

neutrons?

• What subatomic particles make up the nucleus?

Protons, Neutrons, Electrons Practice worksheet

The Periodic Table

Column = Group or Family

18 columns on the Periodic Table

Row = Period

7 rows on the Periodic Table

Lanthanides and actinides are printed belowthe rest of the elements to make the tableeasier to read.

What does the information in the box tell me?

1

H1.008

Atomic Number = # of protons

Atomic Mass = # of

protons plus neutrons

Elemental Symbol

EQ:

•How does the reactivity of metals change across the

periodic table?

Identifying the groups

• Color the alkali metals blue (use pages 132-133) to fill in your periodic table

• Color the alkaline earth metals light green• Color the transition metals yellow• Color the metals in the mixed group purple• Color the actinides dark green• Color the lanthanides orange• Put a yellow circle on the metalloids chemical

symbol

Identifying the groups

• Outline the boron family in pencil• Outline the carbon family members in red• Outline the nitrogen family members in light

blue• Outline the oxygen family members in green• Outline the halogen family members in brown• Outline the noble gases in dark blue• Draw in the stair case in black

Metals, Nonmetals, and Metals, Nonmetals, and Semi-metalsSemi-metals

Metals are to the left of the stair-

step

Onlynonmetal on

the metal sideNonmetals are on the right of the stair-step

Semi-metals,

“metalloids,”

touch the stair-step

Group 1 – The Alkali MetalsGroup 1 – The Alkali Metals

– Most reactive metals on the Periodic Most reactive metals on the Periodic TableTable

• Alkali metals react with other elements by losing one valence electron.

• Most common Na (Sodium) and K (Potassium)

• charge is +1charge is +1

Group 2 – Alkaline Earth MetalsGroup 2 – Alkaline Earth Metals– Still quite reactive. Still quite reactive. – Each is fairly hard, gray-white, and a good

conductor of electricity. – Most common Mg (Magnesium) and Ca (Calcium)

– Like to lose 2 valence electronsLike to lose 2 valence electrons– Charge is +2Charge is +2

• Video on alkali and alkaline earth metals

T he Groups of the Periodic T he Groups of the Periodic TableTable

• Groups 3-12: Transition MetalsGroups 3-12: Transition Metals– Found freely and in compounds in Found freely and in compounds in

naturenature– Charge is usually +2 Charge is usually +2 – Transition metal Video

• Group 13: Boron FamilyGroup 13: Boron Family– Charge is +3 (with 3 valence electrons)Charge is +3 (with 3 valence electrons)

Transition Metals• The elements in Groups 3 through 12 are called

the transition metals .

• The transition metals include most of the familiar metals, such as iron, copper, nickel, silver, and gold.

• Most of the transition metals are hard and shiny.

• All of the transition metals are good conductors of electricity.

• Many of these metals form colorful compounds.

Groups 13-15 (Metals in mixed group, metalloids)

• Only some of the elements in Groups 13 through 15 of the periodic table are metals.

• These metals are not nearly as reactive as those on the left side of the table.

• The most familiar of these metals are aluminum, tin, and lead.

Carbon Family•Each element in the carbon family has atoms that can gain, lose, or share four electrons (+4 or -4) when reacting with other elements.

•In Group 14, only carbon is a nonmetal.

•What makes carbon especially important is its role in the chemistry of life.

•Carbon is found in all living things.

Nitrogen Family

• Nitrogen is an example of an element that occurs in nature in the form of diatomic molecules, as N2.

• A diatomic molecule consists of two atoms.

• In this form, nitrogen is not very reactive.

-3 charge

Oxygen Family• -2 electrons

• Like nitrogen, the oxygen you breathe is a diatomic molecule (O2).

• Oxygen sometimes forms a triatomic (three-atom) molecule, which is called ozone (O3).

• Highly reactive since it can combine with almost every other element.

• Most abundant element in Earth’s crust and the second-most abundant element in the atmosphere. (The first is nitrogen.)

Group 16

• Group 17 contains elements are also known as the halogens , which means “salt forming.”

• The most reactive

non-metals.• A halogen atom typically

has a charge of -1 when

it reacts with other elements.

Halogen Family

Comparing the four halogens video

Noble Gases

• The elements in Group 18 are known as the noble gases .

• They do not ordinarily form compounds because atoms of noble gases do not usually gain, lose, or share electrons.

• The noble gases are usually unreactive.

Inert Gases

Properties of Metals

• Conductivity– Ability to transfer heat or electricity to another object.

• Reactivity– The ease and speed that elements combine (or

reacts) with other elements and compounds.

• Corrosion– Destruction of metal or the gradual wearing away of a

metal element due to a chemical reaction.

Special Rows on the PTSpecial Rows on the PT

Lanthanides

Actinides

Lanthanides

• Two rows of elements are placed below the main part of the periodic table.

• The elements in the top row are called the lanthanides (lan thuh nydz).

• Lanthanides are soft, malleable, shiny metals with high conductivity.

• They are mixed with more common metals to make alloys. An alloy is a mixture of a metal with at least one other element, usually another metal.

Actinides

• The elements below the lanthanides are called actinides (ak tuh nydz).

• All of the elements after uranium in the periodic table were created artificially in laboratories. (Synthetic)– The nuclei of these elements are very unstable,

meaning that they break apart very quickly into smaller nuclei. In fact, many of these elements are so unstable that they last for only a fraction of a second after they are made.

Element 117 videoElement 117 video

Hydrogen• The element with the

simplest and smallest atoms. • Each hydrogen atom has

one proton and one electron. Some hydrogen atoms also have neutrons.

• Because the chemical properties of hydrogen differ very much from those of the other elements, it really cannot be grouped into a family.

• Hydrogen is rarely found on Earth as a pure element. Most hydrogen is combined with oxygen in water (H2O).

+1 charge

Metalloids• Along the border between the metals and the

nonmetals are eight elements called metalloids.

• The metalloids have some characteristics of both metals and nonmetals. – All are solids at room temperature. – They are brittle, hard, and somewhat reactive.

• The most common metalloid is silicon (Si). Silicon combines with oxygen to form silicon dioxide (SiO2). Ordinary sand, which is mostly SiO2, is the main component of glass.

Metalloids Continued

• The most useful property of the metalloids is their varying ability to conduct electricity.

• Whether or not a metalloid conducts electricity can depend on temperature, exposure to light, or the presence of small amounts of impurities.

• Metalloids such as silicon, germanium (Ge), and arsenic (As) are used to make semiconductors.

• Semiconductors are substances that can conduct electricity under some conditions but not under other conditions. Semiconductors are used to make computer chips, transistors, and lasers.

Electrons (e-)

• Electrons move within a sphere-shaped region surrounding the nucleus.

• Scientists depict this region as a cloud of negative charge because electrons may be anywhere within it. – Electrons with lower energy usually move in the

space near the atom’s nucleus. – Electrons with higher energy move within the space

farther from the nucleus.• Most of an atom’s volume is the space in which

electrons move. That space is huge compared to the space taken up by the nucleus.

Light and the Atom

Atoms absorb and then emit energy with their electrons

When the energy emitted falls within the visible spectrum we see it as light

Mendeleev

• Father of the periodic table

• Arranged his periodic table by atomic mass

• Today it is arranged by atomic number

• Mosley later discovered that the periodic nature of the elements was associated with atomic number and not atomic mass.

Isotopes

• See Isotopes ppt

CaCl2 + NaHCO3 ?

What are the reactants?•Calcium chloride: ice melt or driveway “heat”

CaCl2

•Sodium bicarbonate: baking soda

NaHCO3

CaCl2 + NaHCO3 NaCl + CaCO3 + H2CO3

H2CO3 H2O + CO2

heat

What are the products?•Sodium chloride: table

saltNaCl

•Calcium carbonate: chalkCaCO3

•Carbonic acid: found in cola

H2CO3

Obeying the law of conservation of mass

•For a completely correct model, we must be sure that there are equal numbers of each type of atom on left and right side.

CaCl2 + NaHCO3 NaCl + CaCO3 + H2CO3

H2CO3 H2O + CO2

heat

Need to balance equation