Subatomic Particles and Mass, Atomic Numbers and Isotopes

1. What is matter? Anything that occupies space and has mass Has to have both!!!

2. What is an atom? Simplest form of an element How are atoms and elements related? Elements are substances that can not be broken down into different substances

3. How are atoms and elements related? Elements are made of atoms

4. What is this a picture of? water molecule

5 & 6. Based upon the picture A. How many hydrogen atoms are there? 2 B. How many oxygen atoms are there? 1 6. What is the chemical formula? H2O

7. In the formula, where does the # of elements go? After the letter as a subscript H20 Water has how many hydrogens? 2 How do you know? Water has how many oxygens?

8. An atom has three major subatomic particles What is the blue area called? nucleus What is in the blue area? Nucleus -Protons and neutrons What are their charges? Protons (+) neutrons (none) What are the yellow circles? electrons What is its charge? (-) Relationship on periodic table

9. Subatomic particles What has the positive charge? Protons What has a negative charge? Electrons What has no charge? neutrons

11. Atomic # & atomic mass Atomic mass Vs atomic number Atomic # of 6 has 6 protons and 6 electrons Atomic mass = protons + neutrons Atomic mass – atomic # = # of neutrons # of neutrons?

13. Isotopes All carbon How are they different? Different number of neutrons Same mass # How are isotopes used in our lives today? Bone scans

Bonding Why do chemicals bond? To make compounds How do they bond? (look at periodic table) Using electrons in the outer orbitals of an element or atom

1. Where do I find the # of electrons? Top # above the symbol How many electrons are there is Na? 11 How do you know? Above the symbol

2. Finding the number of e- for bonding Look at the top of each column The # represents the amount of electrons in the outer shell orbital

3 & 4. Elements of the left side Vs right side Left are metals Right are non-metals – mostly gases Column 8 = noble gases Why?

5. Ionic Bonds From opposite sides of the periodic table One element is giving up electrons to the other

6. Covalent Bonds From the right side of the periodic table (except for H) One element is sharing electrons with the other

7. Is NaCl an ionic or covalent bond? Why? Different sides of the equation

8. Is CO2 an ionic or covalent bond? Why? Same side of the periodic table

“8” being the magic # except for Hydrogen and helium Look at the atomic # for hydrogen and helium – how many total electrons do they have? Look at the picture How many electrons are in the 1st orbital? How many electrons are in the 2nd orbital?

9. Potassium is in what column? 1st How many electrons are available for bonding? 1

10. Chlorine is in what column? 7 How many electrons are available for bonding?

11. Carbon is in what column? 4 How many electrons are available for bonding?

12. Which elements will bond the easiest and why? A. K B. Cl C. C K and Cl since they only need to add or lose one electron

13. Hydrogen bonding Why is it good for us? Bonds are easily broken Can convert solid to liquid to gas Ice to fluid to condensation Iced tea

14. Balancing Equations Law of Conservation of Mass Reactant and Products must have the same amount of atoms!

Why do we care about atoms, electrons, and bonding in Biology? Why do we eat? To get energy How do we get the energy? Break down food to glucose – every cell in our body needs glucose

Most important elements to Biology CHNOPS Carbon is in all living things (carbon backbone) H2O is in all living things Proteins have Nitrogen and sulfur Phosphorus is in phospholipids