Periodic table
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PERIODIC TABLE. The Language of Chemistry. CHEMICAL ELEMENTS - pure substances that cannot be decomposed by ordinary means to other substances. Aluminum. Bromine. Sodium. The Language of Chemistry. The elements, their names, and symbols are given on the PERIODIC TABLE.

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PERIODIC TABLE

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Periodic table

PERIODIC TABLE


The language of chemistry

The Language of Chemistry

  • CHEMICAL ELEMENTS -

    • pure substances that cannot be decomposed by ordinary means to other substances.

Aluminum

Bromine

Sodium


The language of chemistry1

The Language of Chemistry

  • The elements, their names, and symbols are given on thePERIODIC TABLE


The periodic table

The Periodic Table

Dmitri Mendeleev (1834 - 1907) arranged elements in order of increasing atomic mass.


Groups in the periodic table vertical columns

Groups in the Periodic TableVertical columns

Elements in groups react in similar ways!

Have similar chemical and physical properties


Periods in the periodic table horizontal rows 7

Periods in the Periodic TableHorizontal rows = 7


Regions of the periodic table

Regions of the Periodic Table

3 classes of elements

Metals

Nonmetals

metalloids


Metals

METALS

  • 80% of elements are metals

  • Metallic lust, shiny

  • Good conductors (heat, electricity)

  • Solid at room temperature (except Hg)

  • Ductile – can be pulled through wires

  • Malleable


Nonmetals

NonMetals

  • Most are gases at room temperature

  • Dull color if solid

  • P and S are solids

  • Br - liquid

  • Poor conductors of heat and temperature

    • Carbon is the exception


Metalloids

METALLOIDS

  • Have characteristics of metals and nonmetals

  • Can be metallic

  • Brittle (not malleable or ductile

  • Semiconductors ( Si)


Group 1a alkali metals

Group 1A: Alkali Metals

Silvery colored

Very Reactive

http://www.youtube.com/watch?v=QSZ-3wScePM

Malleable,

ductile

good conductors

soft

Cutting sodium metal


Periodic table

Group 2A: Alkaline Earth Metals

Magnesium

Magnesium oxide

Very reactive


Transition elements

Transition Elements

Lanthanides and actinides

Malleable

Good conductors of electricity and heat

Iron, Cobalt and Nickel can create magnetic

fields

Can have several oxidation (Lose Electrons) states


Group 7a the halogens salt makers f cl br i at

Group 7A: The Halogens (salt makers) F, Cl, Br, I, At

Non Metals

Extremely reactive/Dangerous

Forms salts (NaCl)

Forms Acids (HF)

Used in: lamps (halogen), Teflon (Flourine + Carbon)

http://www.youtube.com/watch?v=u2ogMUDBaf4&feature=related


Group 8a the noble inert gases he ne ar kr xe rn

XeOF4

Group 8A: The Noble (Inert) GasesHe, Ne, Ar, Kr, Xe, Rn

  • Lighter than air balloons

  • “Neon” signs

  • Very Unreactive because they have full electron shells


The periodic table review

The Periodic Table -Review

1. Name group 1

2. Name group 7

3. 2 Characteristics of metals

4. 2 characteristics of nonmetals


Periodic trends

PERIODIC TRENDS

  • Atomic size- Increase in atomic number draws electrons closer to the nucleus = smaller


Ionization energy

Ionization Energy

  • The energy required to remove an electron from an atom in order to form an ion

  • Easy to remove electrons from group 1A more difficult to remove electrons across a row


Periodic table

IONS

  • IONSare atoms or groups of atoms with a positive or negative charge.

  • Taking away an electron from an atom gives a CATION with a positive charge

  • Adding an electron to an atom gives an ANION with a negative charge.

  • To tell the difference between an atom and an ion, look to see if there is a charge in the superscript! Examples: Na+ Ca+2 I- O-2

    Na Ca I O


Forming cations anions

Forming Cations & Anions

A CATION forms when an atom loses one or more electrons.

An ANION forms when an atom gains one or more electrons

F + e- --> F-

Mg --> Mg2+ + 2 e-


Predicting ion charges

PREDICTING ION CHARGES

In general

  • metals (Mg) lose electrons ---> cations

  • nonmetals (F) gain electrons ---> anions


Charges on common ions

-3

-2

-1

+1

+2

Charges on Common Ions

By losing or gaining e-, atom has same number of e-’s as nearest Group 8A atom.


Ionic size

Ionic Size

  • Cations are always smaller than the atoms they form

  • Anions are always larger than the atoms from which they form


Electronegativity

Electronegativity

  • Ability of an atom in an element to attract electrons when the atom is in a compound


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