Thursday, November 15, 2007
Thurs-Day 1
Bio- our classroom became a cell in which we acted out the trait-expressing activities of transcription and translation. We looked at a chromosome, specifically a section of DNA that coded for a trait (curly eye lashes, for example); this section is called a gene or an allele.
We transcribed the gene's DNA to mRNA in the nucleus (at my desk) and then the mRNA travelled from the nucleus (my desk) to the ribosome (your desk) where the tRNA (your lab partner), with the matching tRNA anticodons to the mRNA codons, brought along the amino acids (from the cytoplasm) that were coded for.
If you did the translation correctly, you had the appropriate kinds and sequence of amino acids to form the functional polypeptide/protein (due to its appropriate shape). This protein expressed a trait that transported you to a monetary prize!
We then discussed the point mutations of substitution, addition/insertion, and deletion. Addition and deletion mutations cause frameshift mutations that can drastically alter the amino acid sequence that is coded for; thus, a faulty or lethal protein is made, which kills the cell.
Chem 7-we discussed isotopes of a given element noting that they have the same number of PROTONS (making them atoms of the same element) BUT a different number of NEUtrons. This difference gives the isotopes the same atomic number (# of protons) BUT different mass numbers (which are REALLY the "proton-plus-neutron" numbers!).
Thus, a S-32 atom has 16 protons and 16 neutrons but a S-34 atom has 16 protons and 18 neutrons.
We then discussed the difference between an atom and an ion of a given element. Ions have either more electrons than protons (net negative charge ions, called "anions") or fewer electrons than protons (net positive charge ions, called "cations").
We then did a chart that called for the deduction of various quantities for a given atom bases on the number of each subatomic particles that comprise the atom.
Chem 8/9- We introduced our new unit: Atomic Structure.
We reviewed our past knowledge of what particles comprise an atom, the relative masses and charges of those particles, and the locations of those particles in an atom.
We discussed the terms atom, ion, isotope, atomic number, and mass number. Regular use and application of these terms will help you remember them correctly.
We focused on isotopes of a given element noting that they have the same number of PROTONS (making them atoms of the same element) BUT a different number of NEUtrons. This difference gives the isotopes the same atomic number (# of protons) BUT different mass numbers (which are REALLY the "proton-plus-neutron" numbers!).
Thus, a S-32 atom has 16 protons and 16 neutrons but a S-34 atom has 16 protons and 18 neutrons.
We then discussed the difference between an atom and an ion of a given element. Ions have either more electrons than protons (net negative charge ions, called "anions") or fewer electrons than protons (net positive charge ions, called "cations").
We then did a chart that called for the deduction of various quantities for a given atom bases on the number of each subatomic particles that comprise the atom.
# posted by C @ 6:18 PM 
