Friday, May 9, 2008
Thurs-Day 2
Bio- we began our Ecology unit by looking at the interaction among various populations in a COMMUNITY and between each population and its environment. We defined and gave examples of: organism, population, community, ecosystem, and biome. We then looked at the four necessary factors to maintain a stable ecosystem.
We then focused on some of the ABIOTIC (NON-living) factors that affect an ecosystem.
Chem 7/8- we did several examples of Bronsted acid-base neutralization reactions. In each reaction, we matched up the conjugate acid-base pairs and noted:
1. the acid and base of a conjugate pair look very similar and differ by ONLY ONE H+ !!!
2. a conjugate acid BECOMES its conjugate base partner by DONATING/LOSING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
3. a conjugate base BECOMES its conjugate base partner by ACCEPTING/GAINING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
4. the STRONGER a conjugate acid is, the WEAKER its conjugate base must be.
5. as a reaction proceeds towards equilibrium, there is a shift FROM the stronger acid/stronger base side TOWARDS the weaker acid/weaker base side. Thus, at equilibrium, the concentrations of the weaker acid and weaker base should be higher than the concentrations of the stronger acid
and stronger base.
We also looked at substances that, depending on what substance they are reacting with, can EITHER donate an H+/be a Bronsted acid OR accept an H+/be a Bronsted base; these substances are called AMPHOTERIC (also called) AMPHIPROTIC substances.
We then continued our acidic/basic/neutral salt lab discussion.
Chem 9- we did several examples of Bronsted acid-base neutralization reactions. In each reaction, we matched up the conjugate acid-base pairs and noted:
1. the acid and base of a conjugate pair look very similar and differ by ONLY ONE H+ !!!
2. a conjugate acid BECOMES its conjugate base partner by DONATING/LOSING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
3. a conjugate base BECOMES its conjugate base partner by ACCEPTING/GAINING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
4. the STRONGER a conjugate acid is, the WEAKER its conjugate base must be.
5. as a reaction proceeds towards equilibrium, there is a shift FROM the stronger acid/stronger base side TOWARDS the weaker acid/weaker base side. Thus, at equilibrium, the concentrations of the weaker acid and weaker base should be higher than the concentrations of the stronger acid and stronger base.
We also looked at substances that, depending on what substance they are reacting with, can EITHER donate an H+/be a Bronsted acid OR accept an H+/be a Bronsted base; these substances are called AMPHOTERIC (also called) AMPHIPROTIC substances.
We then focused on some of the ABIOTIC (NON-living) factors that affect an ecosystem.
Chem 7/8- we did several examples of Bronsted acid-base neutralization reactions. In each reaction, we matched up the conjugate acid-base pairs and noted:
1. the acid and base of a conjugate pair look very similar and differ by ONLY ONE H+ !!!
2. a conjugate acid BECOMES its conjugate base partner by DONATING/LOSING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
3. a conjugate base BECOMES its conjugate base partner by ACCEPTING/GAINING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
4. the STRONGER a conjugate acid is, the WEAKER its conjugate base must be.
5. as a reaction proceeds towards equilibrium, there is a shift FROM the stronger acid/stronger base side TOWARDS the weaker acid/weaker base side. Thus, at equilibrium, the concentrations of the weaker acid and weaker base should be higher than the concentrations of the stronger acid
and stronger base.
We also looked at substances that, depending on what substance they are reacting with, can EITHER donate an H+/be a Bronsted acid OR accept an H+/be a Bronsted base; these substances are called AMPHOTERIC (also called) AMPHIPROTIC substances.
We then continued our acidic/basic/neutral salt lab discussion.
Chem 9- we did several examples of Bronsted acid-base neutralization reactions. In each reaction, we matched up the conjugate acid-base pairs and noted:
1. the acid and base of a conjugate pair look very similar and differ by ONLY ONE H+ !!!
2. a conjugate acid BECOMES its conjugate base partner by DONATING/LOSING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
3. a conjugate base BECOMES its conjugate base partner by ACCEPTING/GAINING an H+, therefore the acid-base conjugate pair MUST differ by only one H+.
4. the STRONGER a conjugate acid is, the WEAKER its conjugate base must be.
5. as a reaction proceeds towards equilibrium, there is a shift FROM the stronger acid/stronger base side TOWARDS the weaker acid/weaker base side. Thus, at equilibrium, the concentrations of the weaker acid and weaker base should be higher than the concentrations of the stronger acid and stronger base.
We also looked at substances that, depending on what substance they are reacting with, can EITHER donate an H+/be a Bronsted acid OR accept an H+/be a Bronsted base; these substances are called AMPHOTERIC (also called) AMPHIPROTIC substances.
# posted by C @ 6:41 AM 
