Lecture notes for end of Ch. 1 and start of Ch. 2
Lecture notes for end of Ch. 1 and start of Ch. 2 CHEM 103 - 002
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CHEM 103 - 002
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This 3 page Class Notes was uploaded by Karlee Nelsen on Saturday September 12, 2015. The Class Notes belongs to CHEM 103 - 002 at University of Wisconsin - Eau Claire taught by Sanchita Hati in Fall 2015. Since its upload, it has received 44 views. For similar materials see General Chemistry I in Chemistry at University of Wisconsin - Eau Claire.
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Date Created: 09/12/15
Precision is how constant measurements are Measurements that are close to each other s values are precise Accuracy is how close to the true value the measurements are Scienti c Notation Numerical 39constant ex15 or 59984 only one digit can be to the left of the NXl 7 Signi cant gures determined 1 1 Any nonzero digit is sig 1111 g gt 4SF 2 305L gt 3SF 0023mg gt 2SF 450mL gt3 100kg gt 1 011 Zeros between nonzeros are significant dill Lilljjlll True value Exponential term can be positive or negative a negative number here indicates that N will be smaller when written out and a positive number here indicates the opposite of the negative Zeros to the left of the first nonzero digit aren t significant Zeros to the right of nonzeros digits are significant IF a decimal is present Zeros to the right of last nonzero digit in numbers without a decimal are NOT significant When doing calculations final answers should have the same number of significant figures as the measured number with the fewest number of significant figures ex 75 X 9545 72 Dimensional Analysis used to convert a number in one unit to another unit New Unit 1 New Unit2 NewUnit2 Original unit X EX 250 g x x Original unit New Unit2 1L 32 0zlt lqu 1000 3 943x10 4L cm Ch 2 Atoms Molecules and Ions Protons positive charge p Mass 1672623X103924g Mass 1007 atomic mass units amu u Electrons negative charge e39 0005u Neutrons neutral charge no Atom con guration normal atoms are neutral unless otherwise specified therefore they have the same number of protons as electrons Electron I gt N IAtom lt r eutron 7 gt Nucleus I 7 FProton 1 Atomic number Z is the number of protons in the atom Same elements have the same number of protons Mass number A is the number of protons the number of neutrons The numbers of neutrons are determined from the atomic mass Electron mass is so small that it is negligible in this equation Carbon atomic number 6 protons neutrons C12 isotope 6 6 C 13 isotope 6 7 Oxygen atomic number 8 protons neutrons 016 isotope 8 8 O 17isotope 8 9 o 18 8 10 Isotopes are atoms With the same number of protons but a different number of neutrons Number neutrons mass number atomic number Atomic Weight is the atomic mass of one atom of an element relative to an atom of another the mass of an atom of Carbon 12 6 1 6 12 Atomic unit u 3 A E E6 Atomic I Mass Spectrometer is an instrument used to measure the masses of isotopes and their abundances are determined experimentally by mass spectrometry Uses a device with magnets that can also measure the mass of each individual isotope very precisely The abundances of indiVidual isotopes in mass spectrometry are determined by number of atoms of isotope abundance x 100 total number of atoms of all isotopes of that element b d 39 t l b d 39 t 2 Atomic Weight a un 6111165850 ape Xmassisotopel a un anlcg so ape Xmassisotope2
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