science test!!

how many valence electrons in group 1

1

how many valence electrons in group 2

2

physical properties of Nitrogen family

2 nonmetals: nitrogen and phosphorus 2 metalloids: Arsenic and Antimony 1 metal: Bismuth All solids except Nitrogen which is a gas at room temperature

how many valence electrons in group 13

3

physical properties of Oxygen family

3 nonmetals: Oxygen, Sulfur, and Selenium 2 metalloids: Tellurium and Polonium Oxygen is the only gas, rest are solids at room temperature

how many valence electrons in group 14

4

Chemical Properties/Reactivity of Carbon family

4 valence electrons Moderate reactive, except Carbon which easily bonds with many elements Gain, lose, or share 4 electrons

how many valence electrons in group 15

5

Chemical Properties/Reactivity of Nitrogen family

5 valence electrons Moderately reactive, except nitrogen (not very reactive, very stable) Gain or share 3 electrons

how many valence electrons in group 16

6

Chemical Properties/Reactivity of Oxygen family

6 valence electrons Moderately to highly reactive Oxygen is extremely reactive May gain 2 electrons but often share 2 electrons

how many valence electrons in group 17

7

total of __ periods

7

Chemical Properties/Reactivity of Halogens

7 valence electrons Highly reactive Gain or share 1 electron Never found alone in nature (always bonded to other elements) Often react with alkali metals because they lose 1 electron

how many valence electrons in group 18

8

Chemical Properties/Reactivity of noble gases

8 valence electrons Have full outermost energy level (stable) Inert = non reactive

What pattern do you notice as you move across AND down the table when considering valence electrons?

Across-amount of electrons increases down-amount of electrons increases

The second period at the bottom of the table is called the

Actinides

physical properties of alkaline earth metals

All metals All share metallic properties All solids at room temperature

physical properties of transition metals

All metals Good conductors of heat and electricity Compounds are brightly colored all solids at room temp. except mercury which is a liquid

physical properties of Boron family

All metals except Boron which is a metalloid All solids at room temperature

physical properties of noble gases

All nonmetals All gases All are found in Earth's atmosphere

physical properties of Halogen family

All nonmetals except astatine which is a metalloid Two are gases: fluorine and chlorine One is a liquid; bromine Two solids: iodine and astatine

physical properties of alkali metals

All soft, shiny, silvery, white metals except for Hydrogen All metals are solids at room temperature

physical properties of Carbon family

Begin to change from metals to nonmetals Carbon is a nonmetal Silicon and Germanium are metalloids Tin and Lead are metals All solids at room temperature

The metalloids are

Boron (B) Silicon (Si) Germanium (Ge) Arsenic (As) Antimony (Sb) Tellurium (Te) Polonium (Po)

Chemical Properties/Reactivity of Rare Earth Metals (Lanthanide and Actinide Series)

Can change amount of valence electrons (1, 2, or 3) Medium to low reactivity If react can lose or share 1, 2, or 3 electrons

energy change when an element gains electrons

Electron affinity

Contains one metalloid and 4 metals. Reactive. Aluminum is in this group. It is also the most abundant metal in the earth's crust. (3 outer level electrons)

Group 13: Boron Group

Contains one nonmetal, two metalloids, and two metals. Varied reactivity. (4 outer level electrons)

Group 14: Carbon Group

Contains two nonmetals, two metalloids, and one metal. Varied re-activity. (5 outer level electrons)

Group 15: Nitrogen Group

Contains three nonmetals, one metalloid, and one metal. Reactive group. (6 outer level electrons)

Group 16: Oxygen Group

These metals are extremely reactive and are never found in nature in their pure form. They are silver colored and shiny. Their density is extremely low so that they are soft enough to be cut with a knife. (1 outer level electron)

Group 1: Alkali Metals

Slightly less reactive than alkali metals. They are silver colored and more dense than alkali metals. (2 outer level electrons)

Group 2: Alkaline-earth Metals

All nonmetals. Very reactive. Poor conductors of heat and electricity. Tend to form salts with metals. Ex. NaCl: sodium chloride also known as "table salt". (7 outer level electrons)

Groups 17: Halogens

Unreactive nonmetals. All are colorless, odorless gases at room temperature. All found in earth's atmosphere in small amounts. (8 outer level electrons)

Groups 18: Noble Gases

These metals have a moderate range of reactivity and a wide range of properties. In general, they are shiny and good conductors of heat and electricity. They also have higher densities and melting points than groups 1 & 2. (1 or 2 outer level electrons)

Groups 3 - 12: Transition Metals

Chemical Properties/Reactivity of alkali metals

Have 1 valence electron Highly reactive Easily LOSE 1 electron So reactive never found alone in nature (always bonded to other elements)

Chemical Properties/Reactivity of alkaline earth metals

Have 2 valence electrons Easily LOSE 2 electrons Highly reactive but not as reactive as alkali metals Never found alone in nature (always bonded to other elements) easier to get rid of 2 than to gain 6

determined for the first time the atomic numbers of the elements

Henry Moseley

This element does not match the properties of any other group so it stands alone. It is placed above group 1 but it is not part of that group. It is a very reactive, colorless, odorless gas at room temperature.

Hydrogen

The elements at the bottom of the table were pulled out to keep the table from becoming too long. The first period at the bottom called the

Lanthanides

These are also transition metals that were taken out and placed at the bottom of the table so the table wouldn't be so wide. The elements in each of these two periods share many properties. The lanthanides are shiny and reactive. The actinides are all radioactive and are therefore unstable. Elements 95 through 103 do not exist in nature but have been manufactured in the lab.

Lanthanides and Actinides

organized periodic table by atomic mass

Mendeleev

physical properties of Rare Earth Metals (Lanthanide and Actinide Series)

Part of transition metals Two rows separated out Each row has similar properties Lanthanide series: first row, soft malleable metals that have high luster and conductivity; used to make alloys and high-quality glass Actinide series: second row, all are radioactive

What are valence electrons and why are they so important for understanding chemistry?

Valence electrons are the electrons in the outermost energy level of an atom. The valence electrons indicate the number of electrons that will be lost, gained, or shared in the bonding process and it tells us how an atom will react in a chemical reaction.

Elements in the first group have one outer shell electron and are extremely reactive.

alkali metals

Elements in the second group have 2 outer shell electrons and are also very reactive. They are called

alkaline earth metals

As you move from left to right, metallic properties

become less metallic

Chemical Properties/Reactivity of transition metals

can change amount of valence electrons (1, 2, or 3) Moderately reactive Lose or share 1 2 3 electrons Often corrosive

Atomic size going from left to right

decreases

energy needed to remove an electron going from left to right is

easier to harder

loss of electrons going left to right is

easier to harder

Define ionization energy.

energy needed to remove electrons

The vertical columns on the periodic table are called

groups or families

Elements in group 17 are known as "salt formers". They are called

halogens

Atomic size going down

increases

The periodic table is organized by

increasing atomic number

what trend do you see going from left to right for ionization energy. WHY?

ionization energy increases. As you move across a period, the atom is smaller and the outer electrons are closer to the nucleus and more strongly attracted to the center. it becomes more difficult to remove the outermost electron.

The elements that touch the zigzag line are classified as

metalloids

Most of the elements in the periodic table are classified as

metals

Elements in group 18 are very unreactive. They are said to be "inert". We call these the

noble gases

Which chemical family would be least reactive (least likely to bond with others) and why?

noble gases because their outer electron shell is full

The elements in the far upper right corner are classified as

nonmetals

The horizontal rows on the periodic table are called

periods

Elements in the same family have

similar properties

the periodic law states that

the physical and chemical properties of the elements are periodic functions of their atomic numbers.

The elements in the middle of the table are called "transition" elements because

they are changed from metallic properties to nonmetallic properties.

Elements in groups 3 through 12 have many useful properties and are called

transition metals

electron arrangement in the outermost energy level

valence electrons

Chemical Properties/Reactivity of Boron family

valence electrons Moderately reactive Lose 3 electrons when bonding