Crazy Clue-What Element am I?1. What do dogs do with their bones?2. Storage space for cars3. Half of a dime.4. Lone Ranger’s Horse5. Male member of the Ganese tribe6. A prison inmate that does stand up comedy.7. Superman’s weakness8. What do you do to your clothes when they are

winkled?9. What do you do to your clothes when they are

ripped?10. If someone ate all the cookies on your plate, you

would cry, “They _______.”

Unit: Atomic Theory and Structure

Elements-Pure substances that are all made of the same type of atom

  Represented by chemical symbol  Most are solids at Room Temp.  Earth’s crust made of 92 naturally

occurring elements Building blocks of matter

Alum molecule

John Dalton’s Recommended Chemical Symbols

How symbols were determined: 1.  Use first letter of Name of element 2.  Where conflicts, First letter plus one

additional letter (only capitalize first letter) 3.  Still conflicts, select symbol from Latin

Name

Elements with Latin Chemical SymbolsElement Latin Name Symbol

Gold Aurum Au

Tungsten Wolfram W

Silver Argentum Ag

Lead Plumbum Pb

Potassium Kalium K

Tin Stannum Sn

Sodium Natrium Na

Copper Cuprum Cu

Mercury HydragyrumHg

W = wolfram (tungsten)Cu = cuprum (copper)Au = aurum (gold)Fe = ferrum (iron)Pb = plumbum (lead)Hg = hydragyrum (mercury)K = kalium (potassium)Ag = argentum (silver)Na = natrium (sodium)Sn = stannum (tin)Sb = stibium (antimony)

Atom Smallest piece of matter that still has the

properties of the element All elements made of atoms

Atomic Structure

Protons - (p+) Positive charge Found in nucleus  Mass of 1 amu

amu (atomic mass unit)** Unit of measurement

for atomic particles which is 1/12th the mass of a carbon atom containing 6 protons and 6 neutrons

Neutrons – (no) No charge Found in nucleus Mass of 1 amu

Electrons – (e-) Negative charge Surround the nucleus,

electron cloud No significant mass

“Sub-Subatomic Particles”: Quarks – smaller

particles that make up protons and neutrons

Leptons – smaller particles that make up electrons

Atomic Number The number of protons in an

atom Number of protons also identifies

the element Whole number on Periodic table

No 2 elements have the same atomic number

Atomic #10? Neon

Atomic #9 ? Fluorine

Number of electrons?  If the atom is neutral:

Positives = negatives

# of protons = # of electrons

 

Atomic # = # of electrons

How many Protons and electrons?

Carbon? 6 protons, 6 electrons

Sodium? 11 protons, 11 electrons

Iron? 26 protons, 26 electrons

Mass Number What has mass in atom?

Protons and neutrons the sum of the number of protons and

neutrons in an atom # neutrons = Mass # - Atomic # (protons) Is a whole number for that atom.

How many p+, n0, e-? Lithium –7?

3 p, 4 n, 3 e

Aluminum –27? 13 p, 14 n, 13 e

40K? 19 p, 21 n, 19 e

80Br? 35 p, 45 n, 35 e

Isotopes Atoms of the same element with different

numbers of neutrons Same atomic # but different mass #

3 isotopes of Hydrogen

ProtiumDeuterium Tritium

Isotopes: Different Isotopes have

different properties Carbon – 12 Carbon –

14 Some are

unstable/radioactive

Use for Radioactive Isotopes: Radioactive Dating

Such as Carbon-14 dating Tracers in Medicine I-123 (thyroid

imaging) Radiation Therapy for Cancer Irradiation of foodCobalt-60 Smoke Detectors Americium-241

Ions Charged atom Different number of

protons and electrons No longer neutral

Average atomic mass

On periodic table The weighted average mass

of an element’s isotopes Using Hydrogen

Is closest to the element’s most abundant isotope’s mass number

(if you round the number)Ex. Lithium – 6.941

Lithium – 7 is most abundant

Electron Energy Levels / Orbits each of the 7 energy level can hold a

maximum number of electrons

  Energy Level

Max. # of Electrons

1 2

2 8

3 18

4 18

Each energy level is a different distance from the nucleus

Atoms only have the number of energy levels that are needed for its electrons

Levels closest to the nucleus have lower amounts of energy

Rules for filling energy levels (atomic # 1-18) – Think of Stadium Seating!!

1.  electrons are placed in lowest level first

2.  when level 1 is full then use level 2

3.  fill each shell to capacity until you get to 3rd level (then these rules don’t apply)

Drawing Bohr ModelsOxygen SodiumNeon

Dmitri MendeleevLate 1800 devised the 1st periodic

table Based on elements atomic

mass number at the time only about 63

known elements left spaces in table for

elements yet to be discovered There were some problems

with his table

By arranging the elements in order of increasing atomic weight he discovered that there existed a periodicity of the elemental properties. He used this periodicity to create a table in which that elements with similar properties were vertically aligned with each other.

In making such alignments Mendeleev was able to determine that several, as yet unidentified, elements should exist (the elements with masses 44, 68 and 72 are examples). He went on to make predictions about the properties of these missing elements which aided in their discovery. The discovery of scandium (44), gallium (68) and germanium (72) and examination of their properities (which were very similar to those predicted by Mendeleev) provided evidence for the validity of the periodic table.

Henry Moseley (1913) arranged elements by atomic number rather than atomic mass

Vertical Columns “groups or families”

18 groups Have similar properties Elements have the same

number of electrons in outer energy level

Calledvalence electron #

Modern Table – by increasing atomic #

Horizontal Rows “periods or series” - 7 periods - don’t share similar properties - all elements in the same period have the

same number of electron energy levels

Electron Configurations: 1.Within energy

levels are orbitals or smaller mini orbits

“s” Spherically shaped (2 e-)

“p” dumbbell shaped (6 e-)

“d” double dumbbell (10 e-)

“f” complex (14 e-)

Each orbital has a certain number of sub-orbitals that can each hold up to 2 electrons (that spin opposite each other)

-Rules for filling sub-orbitals: 1. - “s” ALWAYS fills first in any energy level 2. - If it has a “p” then fills after the “s” 3. If it has a “d” orbital, it is always skipped in favor of

the next levels “s” 4. -Then after “s” is filled, go back to the “d” one energy

level lower

2

2

6

26

10

6

2

The Periodic TableContains all the known elements