3. SI Base Units used in Chemistry: Quantity Unit Name Abbreviation Tool to Measure Length Mass Time Temperature Amount of Substance
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1 Honors Chemistry Unit 1 Intro and Atomic Theory Notes Intro Scientific Measurements: 1. Chemistry is the study of. 2. Why do scientists worldwide use the SI system of measurement? 3. SI Base Units used in Chemistry: Quantity Unit Name Abbreviation Tool to Measure Length Mass Time Temperature Amount of Substance 4. What is a derived unit? List 5 examples. 5. What is the purpose of SI prefixes? Why are they useful? 6. Fill out the following table 1 mega (M) 10 6 base Base Meter, liter, gram, second 7. What is a measurement?
2 8. Why are measurements always uncertain? 9. Define: Accuracy Precision Percent Error 10. What is Jake s percent error, if he measured the density of a substance to be 6.8 g/ml during his experiment and the accepted value is 7.2 g/ml? 11. Measure this to the correct digits. Assume these units are ml. 12. Significant figures: Answer 13. Write your approved list of rules below: 14. Use your rules to determine number of sigfigs below: L L x10 5 kg ,000 kg s 15. Multiplying and dividing with sig figs: The number with the fewest sig figs determines the number of sig figs in the answer. Example: 13.91g/cm 3 X 23.3cm 3
3 16. Adding and subtracting with sig figs: The number with the lowest decimal value determines the place of the last sig fig in the answer. Example: 2.65m+5.3m Example: 189L+270L 17. More practice a g 9.1 g b g 0.84g Graphing 1. What is the most common type of graph used in chemistry? 2. When constructing a line graph you should: Direct Proportions Interpreting Relationships from Graphs: Inverse (or Indirect) Proportions Dimensional Analysis 1. What is it used for? 2. What are unit conversions? Examples 3. Convert 13.4 g to mg. 4. Convert 267 kl to L 5. Convert cm to hm 6. Convert 72.7 mph to m/s
4 Density 1. Formula: 2. An object has a volume of 825 cm 3 and a density of 13.6 g/cm 3. Find its mass. Atomic Theory: Matter Pure Substances: The smallest individual unit of an element is called an. Atoms of two or more elements chemically combined make up a. Atomic Structure: Particle Symbol Relative Charge Relative Mass Location in the Atom Proton Neutron Electron The atom consists of three subatomic particles, the,, and. The electron is an elemental particle, whereas the proton and neutron consist of three smaller particles called. Define: Nucleons Atomic Number Mass Number Atomic Mass
5 Isotopes Nuclides Ion Symbolic Notation: What is the atomic number? How many protons? How many neutrons? What is the mass number? How many electrons? Atomic Mass: The average mass system is a relative system based on the mass of a standard nuclide. This nuclide is. The unit for measuring atomic masses is the. Average Atomic Mass: Use the following formula: To calculate average atomic mass Example: Calculate the average atomic mass of boron if a sample contains 19.78% boron-10 (atomic mass = u) 80.22% boron-11 (atomic mass = u) History of the Atom 1. Early Theories of the Atom: a. proposed the first idea of the atom around 430 B.C. b. proposed the first Atomic Theory in Describe this theory:
6 c. Dalton based his theory on the work of two scientists: ( ) Law of Conservation of Mass ( ) Law of Definite Proportions d. Dalton used his theory to develop the Law of Multiple Proportions ( ) 2. Discovery of Subatomic Particles Cathode ray tubes were used to discover two subatomic particles a. ( ) used cathode rays to discover the electron. He measured the bending of the rays to determine the. b. Modified cathode ray tubes were used to discover a beam of positive charge. These rays were determined to be positive particles and were named protons. c. Thomson developed a new model of the atom called the d. ( ) performed the oil drop experiment to determine the charge on the electron. He also used Thomson s charge to mass ratio to calculate the mass of an electron. Describe his experiment: e. The third subatomic particle was discovered much later by ( ). **Discovery of subatomic particles led to the first revision of Dalton s Atomic Theory: Atoms are not indivisible and indestructible; they are made up of smaller particles.** **Discovery of isotopes and neutrons led to the second revision of Dalton s Atomic Theory: Atoms of the same element are NOT exactly alike; they can have the same number of protons, but may have different numbers of neutrons**
7 3. The Nuclear Model of the Atom The nucleus was the next major focus in the development of the atomic model. a. ( ) studied the radiation emitted by these substances, especially the alpha particles. He directed another famous experiment, the gold foil experiment. Describe his experiment: b. Rutherford s model of the atom is called the nuclear model of the atom.
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