2. Check Unit 3 NOTES:
Lesson 1

3. UNIT 3
“ORGANIZING MATTER”

4. MATTER: MATTER is composed of 118 elements with varying properties
everything that has mass (the amount of “matter” that makes up an object), volume (the amount of “space” an object takes up), weight (the amount of “gravity” pushing / pulling on an object) and inertia (resist change in motion)
MATTER is composed of 118 elements with varying properties
REACTIVITY of elements
Very reactive (Groups 1 & 2) form compounds easily
Less reactive
NOT reactive (Group 18 – the INERT / NOBLE Gases)
AND do NOT form compounds

5. PERIODIC TABLE and the ATOM:
Inside the Atom:
NUCLEUS  refers to the “core” of an atom containing the protons (massive, “+” charged subatomic particles) and the neutrons (massive, NO electrical CHARGE particles)
Nucleus is the most massive part of an atom
Atomic Mass Number  refers to the sum of the PROTONS and NEUTRONS found in the nucleus of the atom

6. ATOMIC MASS NUMBER:
Atomic Mass Number  refers to the sum of the PROTONS and NEUTRONS found in the nucleus of the atom
measured in ATOMIC MASS UNITS (amu)
amu’s  refers to the means used by scientists to measure the particles of an atom
the mass of a proton “OR” neutron = “1” amu
a proton or neutron is about 2,000 times more massive than an electron
(e.g.) ATOM with…
3 protons, 4 neutron, and 3 electrons has a mass = “7” amu (3 p + 4 n)

7. FINDING the NEUTRON COUNT:
Use the ATOMIC NUMBER and the AVERAGE ATOMIC MASS NUMBER of an element
SUBTRACT the ATOMIC NUMBER (proton count) from the AVERAGE ATOMIC Mass NUMBER (proton + neutron count of all an element’s atoms and isotopes)
the DIFFERENCE is the neutron count
finally ROUND the decimal fraction to the nearest whole neutron

8. FINDING the NEUTRON COUNT:
(1) (e.g.)
zinc [Zn] Average Atomic Mass # =
Atomic # =
Neutron count =
65.39
- 30
35.39  35
(2) (e.g.)
silver [Ag] Average Atomic Mass # =
Atomic # =
Neutron count =
107.86
- 47
60.86  61
For more practice use the following link and have your calculator ready…

9. ATOMIC MASS NUMBER:
Atomic Mass Number  refers to the sum of the PROTONS and NEUTRONS found in the nucleus of the atom
the MASS number of an element CAN VARY due to the varying number of NEUTRONS the atom of an element can contain
(e.g.) carbon [C] atoms must always contain 6 PROTONS, but can contain anywhere from 5-8 NEUTRONS
Isotopes  are atoms with the same number of PROTONS, but with different numbers of NEUTRONS

10. ATOMIC NUMBER:
all atoms for each element contains the SAME number of PROTONS
(i.e.) all silicon [Si] atoms contain 14
PROTONS
Atomic Number  corresponds to the number of PROTONS an element has
(i.e.) the ATOMIC NUMBER for all
carbon [C] atoms = 6

11. Atomic Number  corresponds to the number of PROTONS an element has
ATOMIC NUMBER VERSUS
ATOMIC MASS NUMBER:
Atomic Number  corresponds to the number of PROTONS an element has
(e.g.) the ATOMIC NUMBER of an element
will NEVER vary
Atomic Mass Number  refers to the sum of the PROTONS and NEUTRONS found in the nucleus of the atom CAN VARY for each atom
measured in ATOMIC MASS UNITS (amu or u)

12. ISOTOPES:
Isotopes  are atoms with the same number of PROTONS, but with different numbers of NEUTRONS
CARBON-12  6 PROTONS and 6 NEUTRONS
Atomic Mass Number = 12 amu
Atomic Number = 6 (protons)
CARBON-14  6 PROTONS and 8 NEUTRONS
Atomic Mass Number = 14 amu

13. ISOTOPES:
Isotopes  are atoms with the same number of PROTONS, but with different numbers of NEUTRONS
HYDROGEN (Protium)  1 PROTON & 0 NEUTRONS
Atomic Mass Number = 1 amu
Atomic Number = 1 (proton)
HYDROGEN (Deuterium)  1 PROTON & 1 NEUTRON
Atomic Mass Number = 2 amu
HYDROGEN (Tritium)  1 PROTON & 2 NEUTRONS
Atomic Mass Number = 3 amu

14. ATOMIC NUMBER, ATOMIC MASS NUMBER and ISOTOPES:

15. Check Unit 3 NOTES:
Lessons 2

16. PERIODIC TABLE:
“PERIODIC”  refers to having a regular, repeating pattern
PERIODS or “rows” ( ) on modern periodic table) align the elements by repeating properties
ELEMENTS in the “PERIODS” are arranged sequentially from LEFT to RIGHT by their ATOMIC NUMBER
ATOMIC NUMBER  refers to the number of PROTONS in the nucleus

17. DMITRI MENDELEEV:
created and published the first PERIODIC TABLE (1869)
organized the elements by the similarities in their physical and chemical properties
arranged the existing elements by their ATOMIC MASS NUMBER
ATOMIC MASS #  is the “average” mass number of one atom of an element
SUM of PROTONS and NEUTRONS
BONDING POWER  refers to the number of bonds an element can form

18. DMITRI MENDELEEV:

19. PERIODIC TABLE: Atomic Number  states the number of PROTONS
basic info per each square for each element includes:
Atomic Number  states the number of PROTONS
Chemical Symbol  abbreviation of an element’s name
Element Name  states the specific element
Relative Atomic MASS Number  the weighted average mass of an element’s atom and all of its isotopes

20. PERIODIC TABLE: Metal / Non-Metal / Metalloid
“PERIODIC” also means “LISTING” & repeating patterns
Periodic Table “LISTS” the elements by:
Metal / Non-Metal / Metalloid
State of Matter (at rm temperature “25o C”) (solid, liquid and gas)
Properties: such as reactivity, number of energy orbitals, number of valence electrons, type of chemical bonding (ionic / covalent)
Atomic Number  the elements gradually change properties as you move from left to right across periodic table as each element gains “one” more proton

21. PERIODIC TABLE: GROUP  term for one of the 18 vertical ( ) columns
Periodic Table “organizes” the elements by “GROUPS” based on having similar characteristics
GROUP  term for one of the 18 vertical ( ) columns
GROUPS  have “family” names based on the first element in that column
(i.e.) Group 14 = CARBON family

22. PERIODIC TABLE:
Periodic Table “organizes” the elements by 18 “GROUPS” based on having similar characteristics

23. PERIODIC TABLE: GROUPS (similar properties):
Group 1 = alkali metals (family name)
from lithium [Li] - francium [Fr]
all metals
very soft
react violently with water
found only in compounds
hydrogen [H] (exception)
*listed with Group 1, but is NOT
an alkali metal

24. PERIODIC TABLE: GROUPS (similar properties):
HYDROGEN (exception to alkali metals)
NOT one of the alkali metals
similar & different properties
simplest element (1 proton & 1 electron)
“1” electron in orbital / valence energy shell
DOES react violently
makes up 90% of the atoms of the universe [due to composition of stars]
makes up only 1% of the mass of the Earth’s crust, oceans and atmosphere

25. PERIODIC TABLE:
Group 1 = alkali metals

26. Group 2 = alkaline earth metals
from beryllium [Be] – radium [Ra]
good conductors of electricity
silvery in color
harder than metals in Group 1
Group 3-12 = transition metals
comprised of 38 “high density” elements
bridge reactive w/ less reactive metals
good conductors of heat & electricity
have luster; are malleable & ductile
contain the familiar metals (Cu, Pb, Ni)
contains iron [Fe] essential to make hemoglobin which carries oxygen [O] in the bloodstream
high melting and boiling points

27. GROUPS 3-12
GROUP 2
Transition Metals
Alkaline Earth Metals

28. PERIODIC TABLE: GROUPS (similar properties): Group 11 = coinage metals
also part of the transition metals
contain the metals (Cu, Au, Ag)
slow to react with water
Group 13-16
include metals, non-metals & metalloids
composed of CARBON family (Group 14),
NITROGEN family (Group 15), and the
OXYGEN family (Group 16)

29. GROUP 14
GROUP 15
CARBON FAMILY
NITROGEN FAMILY

30. GROUP 16
OXYGEN FAMILY

31. Group 18 = noble gases / inert gases
Group 17 = halogen family
from fluorine [F] – astatine [At]
react violently w/ elements from GROUP 1
non-metallic elements
very corrosive
strong odor
in pure form dangerous to humans
in compounds very useful (table salt NaCl)
Group 18 = noble gases / inert gases
from helium [He] – radon [Rn]
rarely react
colorless, odorless, tasteless
very stable elements due to valence energy orbital containing maximum electron count

32. GROUP 17
GROUP 18
HALOGEN FAMILY
NOBLE GASES

33. PERIODIC TABLE: PERIOD  term for one of the “7” horizontal
Periodic Table “organizes” the elements by “PERIODS” which gradually change properties as you move from left to right due to “1” additional proton per element
PERIOD  term for one of the “7” horizontal
( ) rows
PERIOD  number is an indicator of the highest “principle quantum #” for that element
(i.e.) hydrogen [H] (Period 1) = 1s1 orbital
(i.e.) chlorine [Cl] (Period 3) = 3s2 3p5 orbitals

34. PERIODIC TABLE: PERIOD 1 PERIOD 2 PERIOD 3
Periodic table “organizes” the elements by PERIODS which gradually change properties as you move from left to right due to “1” additional proton per element
PERIOD 1
composed of 2 elements: [H] - [He]
both elements have 1 energy orbital
PERIOD 2
composed of 8 elements: [Li] - [Ne]
all 8 elements have 2 energy orbitals
PERIOD 3
composed of 8 elements: [Na] - [Ar]
all 8 elements have 3 energy orbitals

35. PERIODIC TABLE: PERIOD 4 PERIOD 5 PERIODS 6 & 7
Periodic table “organizes” the elements by PERIODS which gradually change properties as you move from left to right due to “1” additional proton per element
PERIOD 4
composed of 18 elements: [K] & [Kr]
all elements have 4 energy orbitals
PERIOD 5
composed of 18 elements: [Rb] - [Xe]
all 18 elements have 5 energy orbitals
PERIODS 6 & 7
each period contains 32 elements and have a portion separated from main body of the periodic table

36. PERIODIC TABLE:
Periodic table “organizes” the elements by PERIODS which gradually change properties as you move from left to right due to “1” additional proton per element

37. PERIODS 6 & 7 (SEPARATED PORTION)
PERIOD 6 (elements 58 – 71) LANTHANIDES:
malleable (easily shaped)
high melting and boiling points
used to make alloys (mixture of metals &/or non-metals)
PERIOD 7 (elements 90 – 103) ACTINIDES:
artificially made in labs; radioactive
unstable since many only last for a fraction of a second
exist in small amounts
(exceptions: thorium [Th] and uranium [U])
LANTHANIDES and ACTINIDES:
also known as “RARE EARTH ELEMENTS” because difficult to isolate

38. LANTHANIDES and ACTINIDES:
also known as “RARE EARTH ELEMENTS”

39. LANTHANIDES and ACTINIDES:
also known as “RARE EARTH ELEMENTS”

40. Check Unit 3 NOTES:
Lesson 3

41. PERIODIC TABLE: Electron Configuration  term for how electrons
additional info per each element square includes:
Electron Configuration  term for how electrons
are arranged within an atom
electron movement around the nucleus is NOT in circular orbits, but in cloud-like zones / “orbitals”
electron location and speed are difficult to predict
“ORBITALS” are grouped and identified according to their shapes: s, p, d, and f (also known as subshells)
“PRINCIPLE QUANTUM NUMBER”  is a whole number which tells the overall energy of the electron and its location
higher the quantum number the more electron energy
farther away from the nucleus the more electron energy
electrons with more energy can occupy different types of orbitals

42. ELECTRON CONFIGURATION:
SHELLS or ENERGY LEVELS are terms often used instead of “PRINCIPLE QUANTUM NUMBER”
if electrons have the same principle quantum number, then those electrons would be in the same energy shell or level
ALL ELECTRONS in the highest principle quantum number orbitals = the number of electrons in the “valence” energy shell
Each orbital can hold a “max” of 2 electrons each:
Type “s” has 1 orbital = TOTAL 2 electrons
Type “p” has 3 orbitals = TOTAL 6 electrons
Type “d” has 5 orbitals = TOTAL 10 electrons
Type “f” has 7 orbitals = TOTAL 14 electrons

43. ELECTRON CONFIGURATION TABLE:
* Shows the amount of electrons different types of orbitals can hold:
Orbital Type
[quantum # (l)]
Number of Orbitals
[(ms) max # of 2 electrons/orbital]
Maximum # of Electrons per Type of Orbital s 1 2 p 3 6 d 5 10 f 7 14

44. ELECTRON CONFIGURATION:
* The order for filling orbitals and electron energy levels:
(Begin at the base of each arrow,
starting with “1 s”, follow it all the
way to the point and begin at the
base of next arrow)
* The order for filling orbitals and energy
levels would be:
1s, 2s, 2p, 3s, 3p, 4s…
* (i.e.) HELIUM [He]
Atomic # =
Electron count =
Electron Configuration =
Stable Atom = 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p 1s
2 (protons)
2 (neutral atom)
1s2
YES 45

45. ELECTRON CONFIGURATION:

46. VALENCE ELECTRONS
Bonding Power  refers to the number of chemical bonds an element can form during a chemical change
electrons explain bonding power because they can either be shared or transferred (given up/taken on) between other atoms
Valence Electrons  are the electrons farthest out from the nucleus and are the ONLY electrons that can be shared or transferred (lost / gained)

47. VALENCE ELECTRONS:
Valence electron energy orbital  name given to the outer-most energy orbital that contains the valence electrons
the amount of valence electron(s) in the valence electron orbital determines whether the atom of an element will share or transfer (give up/take on) electron(s)
the number of valence electron(s) an element has increases from left to right across a period (“row” )

48. VALENCE ELECTRONS by “GROUPS”: Group 1
the elements in each GROUP have the same number and arrangement of valence electrons (outer-most electrons) in their valence electron orbital (outer-most energy subshell)
Group 1
all elements have “1” valence electron
Li – Fr (TRANSFER by “giving” it up)
H (SHARES)

49. VALENCE ELECTRONS by “GROUPS”: Group 2 Group 3-12
the elements in each GROUP have the same number and arrangement of valence electrons (outer-most electrons) in their valence electron orbital (outer-most energy subshell)
Group 2
all elements have “2” valence electrons
TRANSFER by “giving” them up
Group 3-12
all elements have “1 or 2” valence electrons

50. VALENCE ELECTRONS by “GROUPS”: Group 13 [1 “3”] Group 14 [1 “4”]
the elements in each GROUP have the same number and arrangement of valence electrons (outer-most electrons) in their valence electron orbital (outer-most energy subshell)
Group 13 [1 “3”]
all elements have “3” valence electrons
TRANSFER by “giving” them up
Group 14 [1 “4”]
all elements have “4” valence electrons
SHARE; especially carbon [C]

51. VALENCE ELECTRONS by “GROUPS”: Group 15 [1 “5”] Group 16 [1 “6”]
the elements in each GROUP have the same number and arrangement of valence electrons (outer-most electrons) in their valence electron orbital (outer-most energy subshell)
Group 15 [1 “5”]
all elements have “5” valence electrons
TRANSFER by “taking on” 3 electrons
nitrogen [N] will also share (HONC rule)
Group 16 [1 “6”]
all elements have “6” valence electrons
TRANSFER by “taking on” 2 electrons
oxygen [O] will also share (HONC rule)

52. VALENCE ELECTRONS by “GROUPS”: Group 17 [1 “7”]
all elements have “7” valence electrons
TRANSFER by “taking on” 1 electron
SHARE w/themselves making covalent diatomic molecules (i.e. F2, Cl2 Br2, I2)
Group 18 [1 “8”]
all elements have “8” valence electrons (except He has “2” valence electrons)
“stable” elements, therefore do NOT want to SHARE OR TRANSFER their electrons
“INERT” – do NOT bond; do NOT react; do NOT form compounds

53. Determining VALENCE ELECTRON Counts:
(1) count ALL the electrons in the highest
principle quantum number orbital(s)
(e.g.) F = 1s2 2s2 2p5 = “7” valence electrons
Al = 1s2 2s2 2p6 3s2 3p1 = “3” valence electrons
(2) for GROUPS 1, 2, 13 – 18 (except “He”), use
the group number to help determine the
valence electron count
(i.e.) K = GROUP 1  “1” valence electron
Si = GROUP 14  “4” valence electron
Ar = GROUP 18  “8” valence electron
Ca = GROUP 2  “2” valence electron
He = GROUP 18  “2” valence electron

54. VALENCE ELECTRONS by “GROUPS”:

55. Don’t forget to check Lessons (1-2)
THE END
Unit 3; Lesson 3
Don’t forget to check Lessons (1-2)