1. Elements & Atoms with Mr. Khatter

2. Left to right: pure forms of the metals Cobalt, Iron, and Nickel
Elements
The purest form of something – so pure that there’s NOTHING you can do to it to separate it into something else.
Left to right: pure forms of the metals Cobalt, Iron, and Nickel

3. 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.

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

5. Atoms
All matter is composed of small, fast moving particles called atoms. These atoms can join together to form molecules.
This theory is really thousands of individual theories that provide evidence for the whole theory.

6. Atoms
Since the atom is too small to be seen even with the most powerful microscopes, scientists rely upon models to help us to understand the atom.
Believe it or not this is a microscope. Even with the world’s best microscopes we cannot clearly see the structure or behavior of the atom.

7. Scientific Models
Scientists create models to help them to visualize complex properties, structures or behaviors. Since the atom is so small, scientists must gather indirect evidence to develop their models.
This is a model of a very complex molecule made of many different kinds of atoms. Each colored ball represents an atom of a different element.

8. This model (left) represents the most modern version of the atom.
Is this really an Atom?
This model (left) represents the most modern version of the atom.
(Artist drawing)

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
All atoms of the same element have the same number of protons in the nucleus 13
Atomic number Al
Atom symbol
26.981
AVERAGE Atomic Mass

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

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

14. Two isotopes of sodium

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

16. 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 in the steam from a volcano.

17. 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

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

19. 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- _______ _______ _______

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

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

22. Elements & Atoms with Mr. Khatter… The journey continues

23. 10B
11B
AVERAGE ATOMIC MASS
The atomic mass an atom is usually listed underneath the atom’s alphabetical symbol on the periodic table.
The atomic mass is an average of the masses of the atom in its various forms (isotopes).

24. 10B
11B
AVERAGE ATOMIC MASS
Boron exists in its balanced form with 5 protons and 5 neutrons only 20% of the time (as far as we’ve found it in nature so far).
In other words, 20% of the time we have found Boron, it has had an atomic mass of 10.
The other 80% of the time it has an atomic mass of 11, meaning that it has 5 protons and 6 neutrons.

25. 10B
11B
AVERAGE ATOMIC MASS
By knowing that Boron exists with an atomic mass of 10 (5p + 5n) 20% of the time and with an atomic mass of 11 (6p + 5n) 80% of the time, scientists created the following formula to find Boron’s average atomic mass of
(20% x 10) + (80% x 11)

26. AVERAGE ATOMIC MASS
7.5% of the time, Lithium exists as Lithium-6, with 3 protons and 3 neutrons.
The other 92.5% of the time, it exists as Lithium-7, with 3 protons and 4 neutrons.
1.) Write out the equation scientists use to find its average Atomic Mass.

27. AVERAGE ATOMIC MASS 28Si = 92.23%, 29Si = 4.67%, 30Si = 3.10%
Avg. Atomic mass of Si = ______________
AVERAGE ATOMIC MASS
92.23% of the time, Silicon exists as Silicon-28, with 14 protons and 14 neutrons.
4.67% of the time, Silicon exists as Silicon-29, with 14 protons and 15 neutrons.
The other 3.1% of the time, it exists as Silicon-30, with 14 protons and 16 neutrons.
2.) Write out the equation scientists use to find its average Atomic Mass.

28. Quick Check
Complete the sentences below. 3.) Atoms always have an equal number of ____________ and ____________, each of which is equal to the atom’s ____________ number. 4.) Atoms that have unequal numbers of neutrally charged ____________ and positively charged protons are called ____________.

29. Quick Check
Complete the sentences below. 3.) Atoms always have an equal number of protons and electrons, each of which is equal to the atom’s atomic number. 4.) Atoms that have unequal numbers of neutrally charged neutrons and positively charged protons are called isotopes.

30. Electron Organization
The electrons in an atom are organized in energy levels. The levels farther from the nucleus contain electrons that have more energy than levels closer to the nucleus.

31. Electron
Organization

32. Electron
Organization

33. Electron
Organization

34. Electron
Organization

35. Electron Organization
2 electrons – 1st level 8 electrons – 2nd level 8 electrons – 3rd level 5.) Sulfur has an atomic number of 16. How many atoms does it have in each level? Draw a model to answer.

36. 2 – 1st level
8 – 2nd level
6 – 3rd level

37. Electron Organization
2 electrons – 1st level 8 electrons – 2nd level 8 electrons – 3rd level 6.) Magnesium has an atomic number of 12. How many atoms does it have in each level? Draw a model to answer.

38. 2 – 1st level
8 – 2nd level
2 – 3rd level

39. Look at the outermost energy level of each of these atoms
Look at the outermost energy level of each of these atoms. The electrons in an atom’s outermost energy level are called that atom’s valence electrons.

40. Complete these sentences:
7.) Sulfur has _____ valence electrons.
8.) Magnesium has _____ valence electrons.

41. Complete these sentences:
7.) Sulfur has 6 valence electrons.
8.) Magnesium has 2 valence electrons.