Elements and the Periodic table

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Atomic structure

A. Quarks

Hypothetical particles (smallest form of matter)

Proposed in 1963 (Gell- Mann and Zweig)Quarks have fractional chargesCome in six flavorsGrouped together in threes to form almost all subatomic particles

Experimental evidence exist to show ALL six flavors exist

Each quark has an antiquark; antimatter

Gluon is the force that holds quarks together

Subatomic particles (3 types)

1. Proton (+ charge; has mass)

2. Neutron (no charge; has mass)

3. Electron (- charge; has mass BUT very little)

1 and 2 found in the atomic nucleus AND

Accounts for ALL of the atom’s mass

Atomic Terms

A. Atomic Number

Total # of protons in the nucleus

Total # of electrons

Name of the atom (element)

# of protons = # of electrons

B. Atomic Mass Number (AMUs)

# of protons + # of neutrons in the nucleus of the atomIn the periodic table atomic mass number that we see is an average of all the different types of isotopes for that atom (this is why the atomic mass number is not even)

To find the # of neutrons in a atom:

# of neutrons = Atomic Mass # - Atomic #

C. Isotopes

The name, of the atom, remains the same.

Has the same number of protons and electrons.

Has a different number of neutrons.

Some isotopes are radioactive (Radioisotopes)

α β γ emitters

D. Ions

Same number of protons/ neutrons

Different number of electrons (add or remove)

Ions have a “net charge” (either + or -)

Not very stable

# of electrons in the outer most energy level determines how the atom react with other atoms; ∴ the properties of that atom

These electrons have a name:

Valence electrons

Determines the family the element is in.

Name of Element Symbol # of protons # of Neutrons Atomic Mass Atomic Number

Neon Ne 10 20

Cobalt Co 27 59

Gold Au 118 197 79

Chlorine Cl 18 17

Thorium Th 142 90

Lead Pb 82 207

Nickel Ni 28 59

Chromium Cr 28 52

Silicon Si 28

Tungsten W 110

Carbon C 8

Copper Cu 64

Cesium Cs 133

10 1032 27

7917 3590 232

125 8231 28

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Elements- groups of similar atoms with similarproperties

Dimitri Mendeleev (1869)

Looked for patterns based on properties:

Chemical and physical

Atomic mass

Bonding power (form compounds with O2)

Patterns appeared when elements were arranged in order of increasing atomic mass

He also noticed that the bonding power changed in an orderly way

Arranging elements by ↑ AM did not make a perfect table; It left blank spaces

Periodic table (regular, repeating pattern)

Predicted the properties of the “blank spaces”

The current Periodic Table is arranged with two things in mind.Horizontal ROWS:

7 PERIODS- Arrange the elements in order ofincreasing atomic number

Vertical COLUMNS:

18 GROUPSOf these, 8 GROUPS are special FAMILIES

Elements with similar properties

Noble gases

http://chemlab.pc.maricopa.edu/periodic/foldedtable.html

Alkali Metal Family

Never found alone in nature

Valence # is 1

H is NOT a metalSoft metalsCan cut with a knifeSilver and shiny

Highly reactive

Alkaline Earth Metals

Valence # of 2

Slower to react

BUT chemically active

Harder and more dense than family 1Higher MP and BP

Transition MetalsNot a family

Valence # of 1 or 2Most familiar metals Fe, Ni, Cu, Ag, Au

Cu + Zn → Brass

Cu + Sn → Bronze

Sn + Pb → Solder

Au + Cu → 14 karat gold

Boron Family

Carbon Family

Half-way between the reactive metals and non-metals

Over 5 million compounds; Organic chemistry

Nitrogen Family

Oxygen Family

Halogen Gases

Valence # 7

VERY REACTIVE

Poisonous

Noble Gases

Will not react

Inert

http://jersey.uoregon.edu/vlab/elements/Elements.html

Noble gases

http://chemlab.pc.maricopa.edu/periodic/foldedtable.html

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Alien Periodic Table

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Alien Periodic Table

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