The document discusses atomic structure and identification. It explains that all matter is made up of atoms, which are composed of subatomic particles including protons, neutrons, and electrons. Each particle has a different location and charge. Atoms are identified by their atomic number, which is the number of protons, and atomic mass, which is the sum of protons and neutrons. Elements are substances that cannot be broken down further, while compounds are formed from two or more elements bonded together. Mixtures can be either heterogeneous, with noticeably different parts, or homogeneous, with an even distribution making the parts difficult to distinguish.

1. Atomic Structure and
Identification

2. Think about it…
 What is the difference between matter, atoms and
elements???
 Everything is made of matter!!!!!!!!
 An atom is the smallest particle of an element
 An element is something that cant be broken down
into simpler substances.

3. What is this?!??!

4. Electron Configuration
 What does an atom look like?!?!

5. Structure of Atoms
 All matter is made up of many atoms
 Atoms are made of subatomic particles:
 Protons
 Neutrons
 Electrons
 Each of these subatomic particles has its own
charge, location in the atom, and mass

6. Structure of Atoms
Proton Neutron Electron
Location Inside the Inside the Space outside
nucleus nucleus the nucleus
Charge Positive (+) Neutral (no Negative (-)
charge)

7. Identifying Atoms
 Atomic Number

8. Identifying Atoms
 We use atomic numbers to organize
elements on the periodic table
 Atomic number increases from left to right
 The atomic number tells you the number of
protons in an atom
 All elemental atoms have the same number
of protons and electrons!

9. Practice!!!!
 What atom has 22 protons?
 A. Ti
 B. Zr
 C. He
 D. O

10. Practice!!!
 How many protons does Sulfur (S) have?
 A. 15
 B. 16
 C. 17
 D. 18

11. Practice!!!
 The atom with the atomic number of 53 is ______.
 A. Sn
 B. Sb
 C. Te
 D. I

12. Identifying Atoms
 Atomic Mass

13. Identifying Atoms
 Atomic mass (aka atomic weight) is the sum of the
protons and neutrons in the nucleus of that atom
Number of Neutrons = Atomic Mass – Atomic number
 How many protons and neutrons does
Carbon have??
 6 protons
 12 – 6 = 6
 6 neutrons

14. Identifying Atoms
 Sometimes, atoms of the same element have different
atomic masses! These are called isotopes
Atomic Mass
Atomic #
 These atoms are all isotopes of each other. They have the
same number of protons but different number of
neutrons. They are STILL Li atoms!

15. Practice!!!
 How many neutrons does Argon (Ar) have??
 A. 17
 B. 18
 C. 22
 D. 40

16. Practice!!!
 What is the atomic mass of Magnesium (Mg)?
 A. 11
 B. 12
 C. 23
 D. 24

17. Practice!!!
 How many electrons does Phosphorus (P) have?
 A. 15
 B. 30
 C. 46
 D. 106

18. Pure Substance
 A pure substance is matter that always has exactly
the same composition
 A pure substance has a fixed, uniform composition.
 Two categories of substances: elements and
compounds

19. Closer look at Elements!
Elements in Earth’s
Atmosphere

20. Elements
 It cannot be broken down into a smaller substance!
 If it is on the periodic table…its an element!
 No two elements contain the same type of atoms

21. Compound
 What is a compound????
 A compound is made from two or more different
elements that are bonded together

22. Molecule
 A molecule is formed when two or more atoms join
together

23. Mixture
 Mixtures retain some of the
properties of their individual
substances.
 No matter how well you stir the
salsa, the ingredients will not be
evenly distributed. More onions
in one bite.
 Two types of mixtures

24. Heterogeneous Mixture
 In a heterogeneous mixture, the parts of the
mixture are noticeably different from one another

25. Homogeneous Mixtures
 In a homogeneous mixture, the substances are so
evenly distributed that it is difficult to distinguish
one substance in the mixture from another

26. Solution
 Solutions are groups of molecules that are mixed up
in an even distribution.
 They are like homogenous mixtures.
 Think about sugar in water and sand in water.