Monday, December 17, 2007
Mon-Day 2
Bio- UPDATE!!! OUR UNIT EXAM IS ON THURSDAY, DECEMBER 20, 2007; it covers the integumentary system/the skin, the musculo-skeletal system (muscles and bones/skeleton),and locomotion.
HW: Text Ch. 34.3 outline is due on Tuesday (tomorrow).
Today, we reviewed the functions/purposes of skin, muscles, bones, and cartilage. We further discussed the connective tissues: tendons (muscle to bone) and ligaments (bone to bone).
We further discussed and viewed the various diseases (failures to maintain homeostasis) of the skin, muscles, and bones:
skin- dermatitis (excema), melanoma/cancer...see pictures in the posted notes
muscles- muscular dystrophy, the weakening or loss of muscle tissue
ligaments and tendons: tearing of this connective tissue (sprains), tendonitis
bones: arthritis, osteoporosis, gout
Bring in Friday's lab and the completed Sports Injuries handout (check your answers on Blackboard); we will finish up the lab writeup and hand that in tomorrow.
Chem 7/8- we explained the reactivities of metals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to Fr since Fr is the MOST active metal (lowest Zeff and greatest number of OPEL's cause its valence electrons to be weakly held/easily lost/"reacted), but only referring to Zeff and OPEL's will EXPLAIN why one metal is more active than another.
We also explained the reactivities of nonmetals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to F since F is the MOST active nonmetal (very high Zeff (+7) and very low number of OPEL's (2) cause any electrons (from other atoms) that come near its valence shell to be strongly held/easily gained, but only referring to Zeff and OPEL's will EXPLAIN why one nonmetal is more active (gains electrons more easily) than another.
We then compared the sizes of a given metal atom to its stable typical ion. Because the metal atom LOSES electrons to become a CATION, the CATION formed has one LESS OPEL, therefore the cation is SMALLER than the atom that it was made from. This is true for ALL metal atoms that become CATIONS.
We then compared the sizes of a given NONMETAL atom to its stable typical ion. Because the nonmetal atom GAINS electrons to become an ANION, the ANION formed has the same Zeff on those new electrons, the SAME number of OPEL's (because electrons are only added to the VALENCE shell) BUT THERE IS MORE ELECTRON to ELECTRON REPULSION, which spreads out the electrons farther from each other thus making the ANION bigger than the atom from which the anion formed.
Finally, we saw the meaning of the numbers in the chemical formulas of ionic compounds/salts of metal cations with nonmetal anions. We will practice writing the correct formulas for ionic compounds/salts.
Chem 9- we explained the reactivities of metals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to Fr since Fr is the MOST active metal (lowest Zeff and greatest number of OPEL's cause its valence electrons to be weakly held/easily lost/"reacted), but only referring to Zeff and OPEL's will EXPLAIN why one metal is more active than another.
We also explained the reactivities of nonmetals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to F since F is the MOST active nonmetal (very high Zeff (+7) and very low number of OPEL's (2) cause any electrons (from other atoms) that come near its valence shell to be strongly held/easily gained, but only referring to Zeff and OPEL's will EXPLAIN why one nonmetal is more active (gains electrons more easily) than another.
We then compared the sizes of a given metal atom to its stable typical ion. Because the metal atom LOSES electrons to become a CATION, the CATION formed has one LESS OPEL, therefore the cation is SMALLER than the atom that it was made from. This is true for ALL metal atoms that become CATIONS.
We then compared the sizes of a given NONMETAL atom to its stable typical ion. Because the nonmetal atom GAINS electrons to become an ANION, the ANION formed has the same Zeff on those new electrons, the SAME number of OPEL's (because electrons are only added to the VALENCE shell) BUT THERE IS MORE ELECTRON to ELECTRON REPULSION, which spreads out the electrons farther from each other thus making the ANION bigger than the atom from which the anion formed.
Finally, we saw the meaning of the numbers in the chemical formulas of ionic compounds/salts of metal cations with nonmetal anions. We will practice writing the correct formulas for ionic compounds/salts.
HW: Text Ch. 34.3 outline is due on Tuesday (tomorrow).
Today, we reviewed the functions/purposes of skin, muscles, bones, and cartilage. We further discussed the connective tissues: tendons (muscle to bone) and ligaments (bone to bone).
We further discussed and viewed the various diseases (failures to maintain homeostasis) of the skin, muscles, and bones:
skin- dermatitis (excema), melanoma/cancer...see pictures in the posted notes
muscles- muscular dystrophy, the weakening or loss of muscle tissue
ligaments and tendons: tearing of this connective tissue (sprains), tendonitis
bones: arthritis, osteoporosis, gout
Bring in Friday's lab and the completed Sports Injuries handout (check your answers on Blackboard); we will finish up the lab writeup and hand that in tomorrow.
Chem 7/8- we explained the reactivities of metals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to Fr since Fr is the MOST active metal (lowest Zeff and greatest number of OPEL's cause its valence electrons to be weakly held/easily lost/"reacted), but only referring to Zeff and OPEL's will EXPLAIN why one metal is more active than another.
We also explained the reactivities of nonmetals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to F since F is the MOST active nonmetal (very high Zeff (+7) and very low number of OPEL's (2) cause any electrons (from other atoms) that come near its valence shell to be strongly held/easily gained, but only referring to Zeff and OPEL's will EXPLAIN why one nonmetal is more active (gains electrons more easily) than another.
We then compared the sizes of a given metal atom to its stable typical ion. Because the metal atom LOSES electrons to become a CATION, the CATION formed has one LESS OPEL, therefore the cation is SMALLER than the atom that it was made from. This is true for ALL metal atoms that become CATIONS.
We then compared the sizes of a given NONMETAL atom to its stable typical ion. Because the nonmetal atom GAINS electrons to become an ANION, the ANION formed has the same Zeff on those new electrons, the SAME number of OPEL's (because electrons are only added to the VALENCE shell) BUT THERE IS MORE ELECTRON to ELECTRON REPULSION, which spreads out the electrons farther from each other thus making the ANION bigger than the atom from which the anion formed.
Finally, we saw the meaning of the numbers in the chemical formulas of ionic compounds/salts of metal cations with nonmetal anions. We will practice writing the correct formulas for ionic compounds/salts.
Chem 9- we explained the reactivities of metals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to Fr since Fr is the MOST active metal (lowest Zeff and greatest number of OPEL's cause its valence electrons to be weakly held/easily lost/"reacted), but only referring to Zeff and OPEL's will EXPLAIN why one metal is more active than another.
We also explained the reactivities of nonmetals in terms of Zeff on the valence electron(s)
and the number of OPEL's.
We can use the shortcut: on the Periodic Table, the more active metal is located closer to F since F is the MOST active nonmetal (very high Zeff (+7) and very low number of OPEL's (2) cause any electrons (from other atoms) that come near its valence shell to be strongly held/easily gained, but only referring to Zeff and OPEL's will EXPLAIN why one nonmetal is more active (gains electrons more easily) than another.
We then compared the sizes of a given metal atom to its stable typical ion. Because the metal atom LOSES electrons to become a CATION, the CATION formed has one LESS OPEL, therefore the cation is SMALLER than the atom that it was made from. This is true for ALL metal atoms that become CATIONS.
We then compared the sizes of a given NONMETAL atom to its stable typical ion. Because the nonmetal atom GAINS electrons to become an ANION, the ANION formed has the same Zeff on those new electrons, the SAME number of OPEL's (because electrons are only added to the VALENCE shell) BUT THERE IS MORE ELECTRON to ELECTRON REPULSION, which spreads out the electrons farther from each other thus making the ANION bigger than the atom from which the anion formed.
Finally, we saw the meaning of the numbers in the chemical formulas of ionic compounds/salts of metal cations with nonmetal anions. We will practice writing the correct formulas for ionic compounds/salts.
# posted by C @ 11:26 AM 
