Flash Player 9 (or above) is needed to view presentations.
We have detected that you do not have it on your computer. To install it, go here.

Like this presentation? Why not share!

Properties of matter elements compounds and bonding






Total Views
Views on SlideShare
Embed Views



0 Embeds 0

No embeds



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.

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

Properties of matter elements compounds and bonding Properties of matter elements compounds and bonding Presentation Transcript

  • Properties ofMatter, Elements, Comp ounds, and Bonding. 9/14
  • Chemical Properties.A chemical change pemanantly changes the conpoundinto another.Basic unit of matter is an atomSubatomic particles- protons (+), neutrons, and electrons(-)
  • AtomsProtons neutrons in the nucleusElectrons travel around the nucleus in orbits or clouds orlevels of energy.Atom is neither positive or negative in charge - it isneutral.ION- An atom that has lost or gained an electron(s)
  • Identifying ElementsAtomic number- number of protonsThe number of protons (atomic number) determines theidentity of an elementAn element- only one type of atomRepresented by a chemical symbol such as O for oxygenor Na for sodiumCHNOPS- Carbon, Hydrogen, Nitrogen, Oxygen,Phosphorous, Sodium  main elements of human body
  • IsotopesAtoms of the same element that have a different numberof neutronsMany (not all) are unstable and break down, emittingenergy – radioactive isotopesUsed for determining the age of fossils, treatment ofdiseases, and even to sterilize food.
  • Chemical Compounds Compounds- Chemical combination oftwo or more elements Represented by a chemical formula thatindicated the elements in the compoundand their proportions.
  • Chemical BondingIn order to become stable, an atom will either gain, lose,or share electrons. Each level can hold only a certainnumber of electrons. (2,8,8)Ionic, covalent, and polar covalent bond
  • Covalent Bonding Equal Sharing of electrons Each atom fills it’s outermost energy level Smallest particle of a compound is a molecule
  • Ionic BondingAn ionic bond forms whenone atom gains electronsand the other loseselectronsIons are held together bytheir opposite chargesInvolves atoms of verydifferent sizes
  • Chemical reactionsThe making or breaking of bonds is called a chemicalreactionReactants (chemicals that enter a reaction) & products(compounds that are produced)A chemical reaction is indicated by a chemical equation.Na (+) + Cl (-) ---> NaClO2 + 2H2  2H2O
  • Polar CovalentThe unequal sharing between two atoms (usually onemuch larger than the other)Creates slight charge on either side of the molecule.
  • Hydrogen bondBetween hydrogen and another atom such as nitrogen oroxygenWeak attractive force that forms temporary, easily brokenbonds
  • Water importance for living thingsWater has an unusual chemical structureWe are over 70% water
  • Properties of water1. less dense as a solidFound in all three states (solid, liquid and gass) on theearth
  • 2. Water is a good solvent. Many compounds dissolve inwater.3. Water is slow to heat and slow to cool.4. water is cohesive – water molecules will attract othermolecules5. water is adhesive- water adheres to other molecules
  • Why?The bonds are covalent, but the sharing is unequalThe water molecule carries a slight chargeIt is polar
  • Hydrogen BondsThe slight charge attracts other water moleculesThis forms weak temporary hydrogen bonds
  • As water changes state it adds or breaks apart hydrogenbonds. This slows changes in temperature
  • solventSome hydogen bonds will pull strongly enough to break offa hydrogen ionH2O H(+) + OH (-)This will ionize a small portion of the water creating equalnumbers of hydrogen and hydroxide ionssolution (solute and solvent)NaCl  Na+ Cl -
  • In a liter of water only More hydrogen ions are0.0000001 m/l of water has added the ph will go downionized. (That’s 1x10 ^-7) (example hcl)(PH=7) If more hydroxide ions (OH)PH stands for the percent are added then the PH wilof hydrogen ions in solution go up (example. NaOH)in relation to hydroxide ions