• Share
  • Email
  • Embed
  • Like
  • Save
  • Private Content
Chapter 6 1
 

Chapter 6 1

on

  • 1,267 views

 

Statistics

Views

Total Views
1,267
Views on SlideShare
1,267
Embed Views
0

Actions

Likes
1
Downloads
7
Comments
0

0 Embeds 0

No embeds

Accessibility

Categories

Upload Details

Uploaded via as Microsoft PowerPoint

Usage Rights

© All Rights Reserved

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Processing…
Post Comment
Edit your comment

    Chapter 6 1 Chapter 6 1 Presentation Transcript

    • Atoms, Elements and Compounds
    • Atom- building blocks of matter Inside the atom is the nucleus. The nucleus contains protons and neutrons while surrounding the nucleus are the electrons .
    • Electron -> (e - ) ← Electron (e - ) ← Protons & ← Neutrons (p + ) & (n 0 )
      • Protons has a positive charge. (p+)
      • Neutrons has no charge.
      • (n 0 )
      • Electrons has a negative charge. (e-)
      • Since there are protons and neutrons in the atom, the net charge of the nucleus is positive .
      • The nucleus contains most of the mass of the atom.
    • All matter is made up of atoms. Elements - when all the atoms in the matter are the same. There are 118 elements. Ex: Carbon and Oxygen
      • Isotopes- nucleus with the same number of protons but different number of neutrons. This is due to radioactivity.
      • Ex: Carbon Carbon-14
      • 6 protons 6 protons
      • 6 neutrons 8 neutrons
      • Not an isotope Isotope
    • Compounds
      • Compounds - matter that is made up of 2 or more combined elements.
      • Compounds look different than the elements that make them up.
    • Compound Ex:
      • Ex: H & O = H 2 O
      • C & O = CO 2
      • C,H & O = C 6 H 12 O 6
      • 2 Types of Chemical Bonds
      • 1. Ionic
      • 2. Covalent
    • Ionic Bonds
      • Ionic Bonds- the force of attraction between the opposite charges of ions.
      • The giving and taking of electrons (+ with -)
      • Ions - Atoms that have a charge
      • Ex: Magnesium Oxide
      • Mg +2 O -2
      • Mg O = Mg O
      • Ex: Magnesium Chloride
      • Mg +2 Cl -1 2
      • Mg Cl = Cl Mg Cl
      . . .. .. . . .. .. . . . . Ionic Bond . . . . .. .. .. . .. .. .. . .. .. .. .
    • Covalent Bonds
      • Covalent Bond- The attraction that forms between atoms when they share electrons.
      • The sharing of electrons (+ with + or - with -)
      • Molecule - neutral particle formed from covalent bond
      • Ex: Diatomic Chlorine (Cl 2 )
      • Cl -1 Cl -1
      • Cl Cl = Cl Cl
      • Ex: Diatomic Hydrogen (H 2 )
      • H +1 H +1
      • H H = H H
      .. .. .. . .. .. .. . .. .. .. . .. .. .. . . . . . Covalent Bond
    • Van der Waals Forces- attractive forces between the positive and negative regions pull on a molecule and hold them together. Ex: Water The areas of slight positive and negative charge around the water molecules are attracted to the opposite charge of other nearby water molecules. These forces hold water molecules together.
    • http://www.johnkyrk.com/H2O.html
    • atom nucleus proton neutron electron element isotope compound covalent bond molecule ion ionic bond van der Waals force Vocabulary – Section 1 http://science.widener.edu/~svanbram/ptable_6.pdf