Bonds Ionic Covalent Hydrogen. Bonds Ionic Transfer electrons Form between ions (+/-) Covalent Share electrons Weaker than ionic 2 types – Polar – Nonpolar.

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Presentation transcript:

Bonds Ionic Covalent Hydrogen

Bonds Ionic Transfer electrons Form between ions (+/-) Covalent Share electrons Weaker than ionic 2 types – Polar – Nonpolar

Polar Bonds Unequal distribution of charge Water molecule

Nonpolar Equal sharing of electrons

Hydrogen bonds Attraction between positive hydrogen portion of one molecule… And negative portion of a second molecule Water molecules are bonded by hydrogen bonds

Properties of Water Cohesion – Attractive force – Holds together – Due to H-bonding – ex: water sticking to other water molecules-meniscus

Properties of Water Surface tension Related to cohesion Due to H- bonds Cause water to be pulled down into liquid “skin” on top of the water Water striders utube.com/wa tch?v=KSLUw mJOo_M utube.com/wa tch?v=KSLUw mJOo_M

Properties of Water Adhesion – Attractive force between two different surfaces – Ex: Water molecules and glass molecules

Properties of Water Capillary action Raising of liquid Glass tube, water will rise automatically

Acids and Bases

Acids: Taste sour Contains H+, (the more H+, the stronger the acid) Very reactive

Properties of Bases: Taste bitter Contains OH- (the more OH-, the stronger the base) Slippery when wet

Acids and Bases If the number of H + ions in a solution is greater than number of OH - ions than the solution is an acid If the OH - ions are greater than the H + ions than the solution is a base

pH Scale Ranges from 0-14 Numbers 0-6 represent acids 7 is neutral Numbers 8-14 represent bases strongest acid strongest base

pH Scale As you move from pH 0 to pH 14, the concentration of H+ DECREASES (10 times each number) As you move from pH 0 to pH 14, the concentration of OH- INCREASES (10 times each number) Ex: A substance with pH3 is 100 times stronger acid than a substance with pH 5. A substance with pH 8 is 100 times weaker base than a substance with pH 10.

Buffer Neutralize acids or bases Keep the pH from large changes

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