1. Bellwork Pick the handouts off the front table
In your groups, match up the correct parts of an atom and record your answers on the handout

2. Atomic Structure
Chapter 10

3. Standard
SPI Recognize that all matter consists of atoms.

4. I CAN… Identify the different parts of an atom
Draw a correct Bohr model structure of an atom
Explain what an isotope is

5. What is an atom?
Atom: the smallest unit of matter that retains the identity of the substance

6. Atomic Structure Atoms have 2 regions
1) Nucleus: the center of the atom that contains most of the mass of the atom.
2) Electron cloud: surrounds the nucleus & takes up most of the space of the atom.
Nucleus
Electron
Cloud

7. What’s in the Nucleus? In the nucleus we find:
Protons: positively charged subatomic particles
Mass of 1 amu
Neutrons: neutrally charged subatomic particles

8. What’s in the Electron Cloud?
In the electron cloud we find:
Electrons: the subatomic particle with a negative charge and relatively no mass
Mass of ~ 1/1836 amu

9. Subatomic Particles Particle Charge Mass (g) Location Electron (e-) -1
9.11 x 10-28
Electron cloud
Proton (p+) +1
1.67 x 10-24
Nucleus
Neutron
(no)

10. How do we know the number of protons in an atom?
Atomic number (#)= # of protons in an atom
Ex: Hydrogen’s atomic # is 1
hydrogen has 1 proton
Ex: Carbon’s atomic # is 6
carbon has 6 protons
**The number of protons identifies the atom-it’s an atom’s fingerprint.

11. How do we know the number of neutrons in an atom?
Mass #: the # of protons plus neutrons in the nucleus
# of neutrons = mass # - atomic #
Example
Li has a mass # of 7 and an atomic # of 3
Protons = 3 (same as atomic #)
Neutrons= 7-3 = 4 (mass # - atomic #)

12. Mass # vs. Atomic Mass
Mass # ? = The Atomic mass on the periodic table rounded either up or down

13. How do we find the number of electrons in an atom?
Most atoms are neutral (have no overall charge)
Because the only charged subatomic particles are the protons and electrons… they must balance each other out in an electrically neutral atom.
Therefore..
# Electrons = # Protons *
* (in a neutral atom..)

14. Examples He has a mass # of 4 and an atomic # of 2
p+ = 2 no = 2 e- = 2
Cl has a mass # of 35 and an atomic # of 17
p+ = 17, no = 18, e- = 17

15. How exactly are the particles arranged?
Bohr Model of the atom: electron configurations
All of the protons and the neutrons
The 3rd ring can hold up to 8 e-
The 1st ring can hold up to 2 e-
The 2nd ring can hold up to 8 e- 15

16. What does carbon look like?
Mass # = 12 atomic # = 6
p+ = 6 no = 6 e- = 6
6 p and 6 n live in the nucleus 16

17. We’re going to practice drawing Bohr models

18. These are called isotopes.
Atoms of the same element can be different (they can have different # of neutrons)
Thus, different mass numbers.
These are called isotopes.

19. Isotopes are atoms of the same element having different masses, due to varying numbers of neutrons.

20. Hydrogen–1 (protium) 1 Hydrogen-2 (deuterium) Hydrogen-3 (tritium) 2
Isotope
Protons
Electrons
Neutrons
Nucleus
Hydrogen–1
(protium) 1
Hydrogen-2
(deuterium)
Hydrogen-3
(tritium) 2

21. We name the isotope based on its mass number
Naming Isotopes
We name the isotope based on its mass number
carbon-12
carbon-14
uranium-235

22. Isotopes
Elements occur in nature as mixtures of isotopes.

23. Group Work
In your groups, work on the back side of your handout that covers isotopes

24. Exit Ticket
On your post-it, answer #9 on page 273 of the textbook