here we go. i'm going to put my chem and physics notes here. lol. just for fun..
i love the new unit we're doing in physics - Fields, because it uses all the equations and problem solving stuff that you need to know from pretty much the whole year! so it's sort of like a review lol while learning something new.. that's good news for my exam studying, it'll be easier - only if i understand it tho =) & apply the concepts properly, and dont make algebraic mistakes! rawr! they always get me.
anyway, back to september.. here we go.. time machine... beeep.!
These notes are taken from my Gr 12 Chemistry McGrawhill textbook.
An Organic Compound is a compound that is Carbon based, usually contatining C-C and C-H bonds.
The Carbon Atom can form 4 bonds each, all covalent. They can form strong single, double, or triple bonds with other Carbons.
Saturated Molecules only contain single bonds. This means that the Carbon atom is bonded to four other bonds, which makes it saturated, because it can not bond with any more atoms.
Unsaturated Molecules contain double, or triple bonds. This means that the Carbon atom is bonded to three or less bonds, which is not the maximum capacity of atoms it can bond with, therefore being unsaturated.
Electronegativity is a measure of how strongly an atom attracts electrons in a chemical bond.
Bond Dipole: a partial negative and positive charge separated by the length of the bond.
- every polar bond has a bond dipole
- A molecule is polar when the molecule has an overall imbalance of charge.
How to determine Polarity:
Polar: option A - has only one polar bond
option B - has more than one polar bond, but they are placed in positions (specific angles) such that they are not directly opposite from one another, and therefore do not counteract each other.
Non Polar: Option A - has no polar bonds
option B - has more than one polar bond, but they are placed directly opposite from one another, in such a way that they counteract and cancel out.
Shapes: We will only look at four shapes today, but there are lots and lots more T_T in later chapters...
Format: Name - angle, example
Tetrahedral - 109.5 angles, Carbon with 4 single H bonds.
Trigonal Planar (meaning on one plane) - 120, Carbon - Oxygen double bond, and 2 H bonds
Linear - 180, Carbon - Hydrogen double bonds, one on each side of the C atom.
Bent/Angular - 104.5, water, Oxygen atom with two H atoms 104.5 degrees apart, with two lone pairs.
Molecular Formula - gives the total # of atoms in the molecule
Structural Formula - shows # of and types of bonds in their arrangement
Condensed Formula - gives the atoms in the order of which they are attached
i love the new unit we're doing in physics - Fields, because it uses all the equations and problem solving stuff that you need to know from pretty much the whole year! so it's sort of like a review lol while learning something new.. that's good news for my exam studying, it'll be easier - only if i understand it tho =) & apply the concepts properly, and dont make algebraic mistakes! rawr! they always get me.
anyway, back to september.. here we go.. time machine... beeep.!
These notes are taken from my Gr 12 Chemistry McGrawhill textbook.
An Organic Compound is a compound that is Carbon based, usually contatining C-C and C-H bonds.
The Carbon Atom can form 4 bonds each, all covalent. They can form strong single, double, or triple bonds with other Carbons.
Saturated Molecules only contain single bonds. This means that the Carbon atom is bonded to four other bonds, which makes it saturated, because it can not bond with any more atoms.
Unsaturated Molecules contain double, or triple bonds. This means that the Carbon atom is bonded to three or less bonds, which is not the maximum capacity of atoms it can bond with, therefore being unsaturated.
Electronegativity is a measure of how strongly an atom attracts electrons in a chemical bond.
Bond Dipole: a partial negative and positive charge separated by the length of the bond.
- every polar bond has a bond dipole
- A molecule is polar when the molecule has an overall imbalance of charge.
How to determine Polarity:
Polar: option A - has only one polar bond
option B - has more than one polar bond, but they are placed in positions (specific angles) such that they are not directly opposite from one another, and therefore do not counteract each other.
Non Polar: Option A - has no polar bonds
option B - has more than one polar bond, but they are placed directly opposite from one another, in such a way that they counteract and cancel out.
Shapes: We will only look at four shapes today, but there are lots and lots more T_T in later chapters...
Format: Name - angle, example
Tetrahedral - 109.5 angles, Carbon with 4 single H bonds.
Trigonal Planar (meaning on one plane) - 120, Carbon - Oxygen double bond, and 2 H bonds
Linear - 180, Carbon - Hydrogen double bonds, one on each side of the C atom.
Bent/Angular - 104.5, water, Oxygen atom with two H atoms 104.5 degrees apart, with two lone pairs.
Molecular Formula - gives the total # of atoms in the molecule
Structural Formula - shows # of and types of bonds in their arrangement
Condensed Formula - gives the atoms in the order of which they are attached
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