concept:. periodic table group/family period metalloid metal transition element non-metal

ElementsConcept:

Concept: Elements

Periodic tableGroup/family periodMetalloidMetalTransition element

Non-metal

Concept: ElementsLEQ: What are the chemical symbols for the most commonly used elements?

History of Periodic Table

Mendeleev (1869) arranged elements based on atomic mass

Anton van den Broek proposed that elements should be arranged to nuclear charge instead of atomic mass

Moseley confirmed these findings with x-ray spectra and arranged them by atomic number. Therefore, atomic number will increase from left to right.

Concept: ElementsLEQ: What are the chemical symbols for the most commonly used elements?

H - Hydrogen Li - Lithium Na - Sodium K - Potassium Be -Beryllium Mg - Magnesium Ca - Calcium Ba – Barium Fe - Iron Ni – Nickel Pt - Platinum Cu - Copper Ag -Silver Au – Gold Zn - Zinc Hg - Mercury B - Boron Al – Aluminum C - Carbon

Si - Silicon Ge – Germanium Sn - Tin Pb - Lead N - Nitrogen P - Phosphorus As -Arsenic Sb - Antimony Bi – Bismuth O - Oxygen S - Sulfur Se - Selenium F - Fluorine Cl - Chlorine Br - Bromine I - Iodine He - Helium Ar - Argon Kr –Krypton Ne – Neon

Concept: ElementsLEQ: What are the distinguishing characteristics of metals, nonmetals, and metalloids?

Metals (blue area; groups 1-12 except H, and

under stair-step line groups 13-15) Good conductors of heat and electricity Solid at room temperature (except for

Hg) Reflects light (luster) Malleable (hammered into sheets) Ductile (stretched/drawn into wire)


Alkali Metals Group 1 (one valence electron) Softer than most other metals Silvery/shiny Most reactive of all metals (reacts

rapidly with oxygen and water) Do not occur in nature in elemental form Stored (kerosene) Fr - radioactive


Alkaline Earth Metals Group 2 (2 valence electrons) Not found as free elements in nature Gives fireworks color, bright red

lights, aircraft


Transition elements Groups 3-12 (elements in transformation) Form colored compounds Often occur in nature as uncombined

elements “Iron Triad” (Fe, Co, Ni – 8, 9, 10)

Used to make steel and other metal mixtures “Coinage Metals” (Cu, Ag, Au – 11)

Stable, malleable, found in nature as free elements


Zn, Cd, Hg (group 12) Used to coat other metals Cd – rechargeable batteries Hg – liquid thermometers


Inner Transitional Metals ALL are radioactive and unstable Lanthanides (Atomic Number 58-71) Actinides (Atomic Number 90-103)


Nonmetals Gases or brittle solids at room temperature Can form ionic or covalent bonds Not malleable Not ductile Most do not conduct heat or electricity Generally not shiny All, except H, are found on right of periodic

table (in yellow)


Group 17 “Halogens” Most reactive non-metal 7 electrons in outer nrg level, one needed to

make it complete Gains an electron from metal forms a salt In gaseous state form reactive diatomic

covalent molecules (identified by distinctive colors)

F – most chemically active of all elements Cl – most abundant halogen Br – only nonmetal that is liquid at room temp


Group 18 “Noble gases” Full outer energy level “happy” so

they exist as isolate atoms Stable & Relatively unreactive


Metalloids Elements along stair-step line

(except for Al) Can form ionic and covalent bonds

with other elements metallic and nonmetallic properties Semiconductors


Mixed groups Group 13 – Boron Group (Al most

abundant metal) Group 14 – Carbon group Group 15 – Nitrogen Group Group 16 – Oxygen Group


Synthetic Elements Elements not typically found on

Earth Made in a lab With exception to Technetium 43 and

Promethium 61, each synthetic element has more than 92 protons


Plutonium (94) used in bombs and control rods of nuclear reactors

Americium – smoke detectors

Transuranium Elements – elements with 92+

Synthetic and unstable; disintegrate quickly

Not considered metals, nonmetals, or metalloids

Concept: ElementsLEQ: How does an element’s location on periodic table relate to valence electrons?

Period Horizontal rows (across) Use to tell energy level

Group Vertical columns (down) Elements within a group have similar properties due to valence

electrons Use to tell valence electrons

Valence electrons the electrons in the outer most energy level that are available

to chemically react Correlates to the group number for main group elements


Energy levels (nrg)

1-7 Correlate to periods (rows) on table 1st nrg level can only hold 2 e. 8 e are

needed for each nrg level to make that level complete and stable. Nrg levels closest to nucleus have lower nrg

Level 1 up to 2 e Level 2 up to 8 e Level 3 up to 18 e Level 4 up to 32 e


Valence electrons for main group elements

Group 1 – 1; give up 1 Group 2 – 2; give up 2 Group 13 – 3; give up 3 Group 14 - 4 Group 15 – 5; gain 3 Group 16 – 6; gain 2 Group 17 – 7; gain 1 Group 18 – 8; gain 0


Electron cloud structure

Lewis Dot structure

concept:. periodic table group/family period metalloid metal transition element non-metal

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