1. Draw what you think an atom looks like, in your notebook. 2. What is an element? Are there different kinds? How many?

1. What is the difference between a compound and an element? 2. What is an atom made of?

1. Were atoms involved in it going out? Why or why not? 2. Why did the flame go out?

 Atom is the smallest unit of matter  Atoms make up all matter, anything that has mass and takes up space.

 Atoms are made up of three different pieces: Protons (positive charge) Electrons (negative charge) Neutrons (no charge)

 An element is something that is made up of one type of atom.  All elements can be found on the periodic table.

 What do you think makes each element different?  What are some examples of elements you know of?

 An ion is an atom that has become either positively or negatively charged.  This usually happens when an atom gains or loses an electron.

 An ion is an atom that has become either positively or negatively charged.  This usually happens when an atom gains or loses an electron.

 Bonds bind one atom to another.  There are three main types of bonds when we are talking about atoms: Ionic bonds Covalent bonds Hydrogen bonds

 Ionic bonds form when one ion is attracted to the another ion.  Ionic bonds are like magnets being attracted to each other. Opposites Attract!

 Ionic bonds form when one ion is attracted to the another ion.  Ionic bonds are like magnets being attracted to each other.

 Covalent bonds form when two neutral atoms share electrons to complete their outer shell.  Atoms want to have 8 electrons in their outer shell. They will bond to make it happen.

 Hydrogen bonds are formed between hydrogen ions and other ions.  They form between a positive hydrogen ion and a negative ion.  Again opposites attract

 What is the difference between a covalent and iconic bond?  Where do you think we normally find hydrogen bonds?

1. Explain why covalent bonds are so much stronger than ionic bonds. 2. If I take one electron away from sodium (Na) what does it become? Why?

 Hydrogen bonds are most commonly found in water.  The negative oxygen ions pull on other positive hydrogen ions in water.

 Water is a polar molecule because of its hydrogen bonds.  Polar means that is has two oppositely charged sides or poles.

 The hydrogen bonds (polar) give water unique properties: Cohesion Adhesion Specific heat capacity Universal solvent

 Cohesion is the ability of water to stick to itself really well. This causes what's referred to as water tension.

 Adhesion is the ability for water to stick to other things really well.

 Specific heat capacity is waters resistance to changing temperature.  This is very useful in keeping temperatures steady in our own bodies.

 Water is also a universal solvent.  This means that most solutes (solids) that are mixed in water, break down.  Like dissolves like, it cannot break down non-polar molecules

 The pH scale runs from 1-14  is a acid  7.1 – 14 is a basic, what is missing?  7 is actually a neutral

1. Pick one water property, explain it in detail. 2. What do you think pH stands for? 3. What do you think the difference is between a solvent and a solute?

 The atomic number is the amount of protons that an element has.  The atomic mass is the number of protons plus the number of neutrons.

 How many protons does this element have?  How many neutrons?

 Give me a short 3-4 sentence summary about what you learned today.  Give me another sentence on somewhere one of these things applies to your world.