1. Elements, Atoms, and Ions
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2. The Language of Chemistry
CHEMICAL ELEMENTS -
pure substances that cannot be decomposed by ordinary means to other substances.
Aluminum
Bromine
Sodium

3. The Language of Chemistry
The elements, their names, and symbols are given on the PERIODIC TABLE
How many elements are there?

4. The Periodic Table
Dmitri Mendeleev ( )

5. Glenn Seaborg (1912-1999 ) Discovered 8 new elements.
Only living person for whom an element was named.

6. The Atom nucleus (of protons and neutrons)
An atom consists of a
nucleus
(of protons and neutrons)
electrons in space around the nucleus.
Electron cloud
Nucleus

7. Copper atoms on silica surface.
An _____ is the smallest particle of an element that has the chemical properties of the element.
Copper atoms on silica surface.
Distance across = 1.8 nanometer (1.8 x 10-9 m)

8. Subatomic Particles He Quarks component of protons & neutrons 6 types
3 quarks = 1 proton or 1 neutron

9. ATOM COMPOSITION The atom is mostly empty space
protons and neutrons in the nucleus.
the number of electrons is equal to the number of protons.
electrons in space around the nucleus.
extremely small. One teaspoon of water has 3 times as many atoms as the Atlantic Ocean has teaspoons of water.

10. ATOMIC COMPOSITION Protons (p+) Electrons (e-) Neutrons (no)
+ electrical charge
mass = x g
relative mass = atomic mass units (amu) but we can round to 1
Electrons (e-)
negative electrical charge
relative mass = amu but we can round to 0
Neutrons (no)
no electrical charge
mass = amu but we can round to 1

11. Atomic Number, Z
All atoms of the same element have the same number of protons in the nucleus, Z 13
Atomic number Al
Atom symbol
26.981
AVERAGE Atomic Mass

12. Mass Number, A Mass Number (A) = # protons + # neutrons
C atom with 6 protons and 6 neutrons is the mass standard
= 12 atomic mass units
Mass Number (A) = # protons + # neutrons
NOT on the periodic table…(it is the AVERAGE atomic mass on the table)
A boron atom can have A = 5 p n = 10 amu

13. CHEMICAL COMPOUNDS are composed of atoms and so can be decomposed to those atoms.
The red compound is composed of • nickel (Ni) (silver) • carbon (C) (black) • hydrogen (H) (white) • oxygen (O) (red) • nitrogen (N) (blue)

14. Compounds composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)

15. A MOLECULE is the smallest unit of a compound that retains the chemical characteristics of the compound.
Composition of molecules is given by a MOLECULAR FORMULA
H2O
C8H10N4O2 - caffeine

16. ELEMENTS THAT EXIST AS DIATOMIC MOLECULES
Remember:
HONClBrIF or
BrINClHOF
These elements only exist as PAIRS. Note that when they combine to make compounds, they are no longer elements so they are no longer in pairs!

17. Dalton’s Atomic Theory
John Dalton ( ) proposed an atomic theory
While this theory was not completely correct, it revolutionized how chemists looked at matter and brought about chemistry as we know it today instead of alchemy
Thus, it’s an important landmark in the history of science.

18. Dalton’s Atomic Theory - Summary
matter is composed, indivisible particles (atoms)
all atoms of a particular element are identical
different elements have different atoms
atoms combine in certain whole-number ratios
In a chemical reaction, atoms are merely rearranged to form new compounds; they are not created, destroyed, or changed into atoms of any other elements.

19. Problems with Dalton’s Atomic Theory?
1. matter is composed, indivisible particles
Atoms Can Be Divided, but only in a nuclear reaction
2. all atoms of a particular element are identical
Does Not Account for Isotopes (atoms of the same element but a different mass due to a different number of neutrons)!
3. different elements have different atoms
YES!
4. atoms combine in certain whole-number ratios
YES! Called the Law of Definite Proportions
5. In a chemical reaction, atoms are merely rearranged to form new compounds; they are not created, destroyed, or changed into atoms of any other elements.
Yes, except for nuclear reactions that can change atoms of one element to a different element

20. Isotopes
Atoms of the same element (same Z) but different mass number (A).
Boron-10 (10B) has 5 p and 5 n
Boron-11 (11B) has 5 p and 6 n
10B
11B

21. Figure 3.10: Two isotopes of sodium.

22. Isotopes & Their Uses
Bone scans with radioactive technetium-99.

23. Isotopes & Their Uses
The tritium content of ground water is used to discover the source of the water, for example, in municipal water or the source of the steam from a volcano.

24. Atomic Symbols
Show the name of the element, a hyphen, and the mass number in hyphen notation
sodium-23
Show the mass number and atomic number in nuclear symbol form
mass number
23 Na
atomic number

25. Isotopes?
Which of the following represent isotopes of the same element? Which element?
234 X X 235 X 238 X

26. Counting Protons, Neutrons, and Electrons
Protons: Atomic Number (from periodic table)
Neutrons: Mass Number minus the number of protons (mass number is protons and neutrons because the mass of electrons is negligible)
Electrons:
If it’s an atom, the protons and electrons must be the SAME so that it is has a net charge of zero (equal numbers of + and -)
If it does NOT have an equal number of electrons, it is not an atom, it is an ION. For each negative charge, add an extra electron. For each positive charge, subtract an electron (Don’t add a proton!!! That changes the element!)

27. MODERN ATOMIC THEORY

28. Chemical Symbols
There are about a dozen common elements that have a single capitalized letter for their symbol
The rest, that have permanent names have two letters.
the first is capitalized and the second is lower case.
Some elements have symbols from their Latin names.
Ten of the elements have symbols from their Latin or German names.

29. Symbols and Atomic Structure
A molecule is a particle that is composed of two or more atoms held together by a chemical bond.
Isotopes are atoms of an element with identical chemical properties, but different masses due to a difference in the number of neutrons.
The atomic mass of an element is the average of all the atomic masses of the isotopes.
an isotopes contribution is determined by its relative abundance.

30. The mass of an element is the mass of the element compared to an isotope of carbon Carbon 12.
Carbon 12 is assigned an atomic mass of g.
12.00 is one atomic mass unit
The number of protons and neutrons in an atom is its mass number.
Atomic numbers are whole numbers
Mass numbers are whole numbers
The atomic mass is not a whole number.

31. Charge (if ion)
Atomic Mass
Symbol
Atomic Number

32. Hydrogen
Protons: 1
Neutrons: 0
Electrons: 1 H 1 1

33. Sodium
Protons: 11
Neutrons: 12
Electrons: 11 Na 23 11

34. Rhenium
Protons: 75
Neutrons: 111
Electrons: 75 Re
186 75

35. Rhenium isotope
Protons: 75
Neutrons: 112
Electrons: 75 Re
187 75

36. Cs 133 55 EXAMPLE Atomic number = protons and electrons
How many protons, neutrons and electrons are found in an atom of
133 55 Cs
Atomic number = protons and electrons
There are 55 protons and 55 electrons
Mass number = sum of protons and neutrons
133 – 55 = 78
There are 78 neutrons

37. Learning Check – Counting
Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of these carbon atoms.
12C C 14C
#p+ _______ _______ _______
#no _______ _______ _______
#e- _______ _______ _______

38. Answers
12C C 14C #p
#no #e

39. Learning Check An atom has 14 protons and 20 neutrons.
A. Its atomic number is
1) ) ) 34
B. Its mass number is
C. The element is
1) Si 2) Ca 3) Se
D. Another isotope of this element is
1) 34X 2) 34X 3) 36X

40. IONS
IONS are 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

41. 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 --> Mg e-

42. PREDICTING ION CHARGES
In general
metals (Mg) lose electrons ---> cations
nonmetals (F) gain electrons ---> anions

43. Learning Check – Counting
State the number of protons, neutrons, and electrons in each of these ions.
39 K O Ca +2
#p+ ______ ______ _______
#no ______ ______ _______
#e- ______ ______ _______

44. One Last Learning Check
Write the nuclear symbol form for the following atoms or ions:
A. 8 p+, 8 n, 8 e- ___________
B. 17p+, 20n, 17e- ___________
C. 47p+, 60 n, 46 e- ___________

45. Charges on Common Ions -3 -2 -1 +1 +2
By losing or gaining e-, atom has same number of e-’s as nearest Group 8A atom.

46. 10B
11B
AVERAGE ATOMIC MASS
Because of the existence of isotopes, the mass of a collection of atoms has an average value.
Boron is 20% 10B and 80% 11B. That is, 11B is 80 percent abundant on earth.
For boron atomic weight
= (10 amu) (11 amu) = amu

47. Isotopes & Average Atomic Mass
Because of the existence of isotopes, the mass of a collection of atoms has an average value.
6Li = 7.5% abundant and 7Li = 92.5%
Avg. Atomic mass of Li = ______________
28Si = 92.23%, 29Si = 4.67%, 30Si = 3.10%
Avg. Atomic mass of Si = ______________

48. The Periodic Table

49. Periods in the Periodic Table- periods are horizontal rows

50. Groups in the Periodic Table- groups are vertical columns
Elements in groups react in similar ways!

51. Introduction
The periodic table is made up of rows of elements and columns.
An element is identified by its chemical symbol.
The number above the symbol is the atomic number
The number below the symbol is the rounded atomic weight of the element.
A row is called a period
A column is called a group

52. Regions of the Periodic Table

53. Group 1A: Alkali Metals Reaction of potassium + H2O
Cutting sodium metal

54. Group 2A: Alkaline Earth Metals
Magnesium
Magnesium oxide

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

56. Group 8A: The Noble (Inert) Gases He, Ne, Ar, Kr, Xe, Rn
Lighter than air balloons
“Neon” signs
Very Unreactive because they have full electron levels
XeOF4

57. Transition Elements Iron in air gives iron(III) oxide
Lanthanides and actinides
Iron in air gives iron(III) oxide

58. Periodic Table
This table is a remarkable way to show the relationships between differing kinds of elements
The modern table was devised (made) in 1869 by Dimitri Mendeleyev
He arranged the elements by weight and by their chemical properties
"...if all the elements be arranged in order of their atomic weights a periodic repetition of properties is obtained." - Mendeleyev

60. The Modern Periodic Table

61. Periodic Patterns
The chemical behavior of elements is determined by its electron configuration
Energy levels are quantized so roughly correspond to layers of electrons around the nucleus.
A shell is all the electrons with the same value of n.
n is a row in the periodic table.
Each period begins with a new outer electron shell

62. Each period ends with a completely filled outer shell that has the maximum number of electrons for that shell.
The number identifying the A families identifies the number of electrons in the outer shell, except helium
The outer shell electrons are responsible for chemical reactions.
Group A elements are called representative elements
Group B elements are called transition elements.

63. Chemical “Families”
IA are called alkali metals because the react with water to from an alkaline solution
Group IIA are called the alkali earth metals because they are reactive, but not as reactive as Group IA.
They are also soft metals like Earth.
Group VIIA are the halogens
These need only one electron to fill their outer shell
They are very reactive.
Group VIIIA are the noble gases as they have completely filled outer shells
They are almost non reactive.

64. Four chemical families of the periodic table: the alkali metals (IA), the alkaline earth metals (IIA), halogens (VII), and the noble gases (VIIIA).

65. Non-Metal: Elements in the upper right corner of the periodic
Metal: Elements that are usually solids at room temperature. Most elements are metals.
Non-Metal: Elements in the upper right corner of the periodic
Table. Their chemical and physical properties are different
from metals.
Metalloid: Elements that lie on a diagonal line between the
Metals and non-metals. Their chemical and physical
properties are intermediate between the two.

66. When an atom or molecule gain or loses an electron it becomes an ion.
A cation has lost an electron and therefore has a positive charge
An anion has gained an electron and therefore has a negative charge.

67. Elements with 1, 2, or 3 electrons in their outer shell tend to lose electrons to fill their outer shell and become cations.
These are the metals which always tend to lose electrons.
Elements with 5 to 7 electrons in their outer shell tend to gain electrons to fill their outer shell and become anions.
These are the nonmetals which always tend to gain electrons.
Semiconductors (metalloids) occur at the dividing line between metals and nonmetals.

68. EXAMPLE So the charge would be +1
What would the charge be on a sodium ion?
Since sodium in in Group IA it is a metal and so would
LOSE an electron
You can tell how many would be lost by the group number
Group 1A elements lose 1 electron
So the charge would be +1
Remember an electron is negatively charged. When you lose them atom becomes positively charged…
when you gain them it becomes negatively charged

69. Na +1 EXAMPLE It has 1…remember the group number!
How would you right the symbol for the sodium CATION? Na +1
How many outer electrons does sodium have before it loses one?
It has 1…remember the group number!

70. Rutherford’s experiment.

71. The modern view of the atom was developed by Ernest Rutherford (1871-1937).

72. Results of foil experiment if Thomson’sPlum Pudding model had been correct.

73. What Actually Happened