sig figs
Conversions
Properties
Definitions
Miscellaneous
100
How many significant figures are in the number 720?
2
100
Convert 3590nm to m
3.59 x 10-6 meters
100
Draw on the board: the difference between precision and accuracy.
Drawn...
100
Define Atom
The smallest particle of an element that retains the chemical characteristics of that element. Elements are the basic building blocks of matter. These are all shown in the Periodic Table.
100
How many neutrons does Fe 2+ have
30 neutrons
200
How many significant figures are in the number 0.00300?
3
200
How many inches are in 1.00 km?
39,400in
200
Name 3 things for each category: -Elements -homogenous mixture -heterogenous mixture -compounds
200
Define molecule
A group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction.
200
On the board, correctly write the symbol of an element with the mass and atomic numbers shown: Carbon 14
Drawn...
300
Complete the following calculation using the proper number of significant figures: 2.34 - 1.293
1.05
300
A bar is 400cm long. How many meters is it?
4 meters
300
Terms of defining phase changes: (1/2 point each) a. Sublimation = b. Deposition = c. Melting = d. Freezing = e. Vaporization = f. Condensation =
a) solid to gas b) gas to solid c) solid to liquid d) liquid to solid e) liquid to gas f) gas to liquid
300
What is an ionic compound and give an example
Made of a metal and a nonmetal.
300
What are the characteristics of the metals, nonmetals, and metalloids.
* Metals = They are characterized by bright luster, hardness, ability to resonate sound and are excellent conductors of heat and electricity. Metals are solids under normal conditions except for Mercury. * Nonmetals= Elements that tend to gain electrons to form anions during chemical reactions are called non-metals. These are electronegative elements. They are non-lustrous, brittle and poor conductors of heat and electricity (except graphite). Non-metals can be gaseous, liquids or solids. * Metalloids = semi-conductors, shiny, brittle
400
Complete the following calculation using the proper number of significant figures: (8.41 X 2.873) + 4.77
29.0
400
Convert 74 degrees F to C
23 degrees C
400
Identify the difference between intensive and extensive properties. Give 2 examples of each.
-An extensive property is a property that changes when the size of the sample changes. Examples = mass, volume, length, and total charge. -An intensive property doesn't change when you take away some of the sample. Examples = temperature, color, hardness, melting point, boiling point, pressure, molecular weight, and density
400
How do matter and mass differ?
Matter is the stuff in the universe. To be more exact, matter is material that occupies space and has mass. Mass is how we measure the amount of matter, and scientists like to use kilograms
400
Explain the differences between the scientists Thomson, Millikan, Rutherford, and Chadwick. What were their experiments and what are they known for discovering.
-Thomson: Cathode ray tube experiment Discovered the electron (negatively charged) Determined the mass/charge ratio of an electron -Millikan: oil drop experiment Determined the charge on an electron Determined the mass of an electron -Rutherford: Gold foil experiment Used radioactivity (alpha particles, these are protons) Determined the positive charged particles were clustered together, called this the nucleus -Chadwick: Used alpha particles and identified neutrons, also located in the nucleus
500
Complete the following calculation using the proper number of significant figures: (9.56 + 87.005)/9.234
10.46
500
The density of a penny minted after 1983 is 7.18 g/cm3. What is the average volume of a penny if the mass of 1 x 105 pennies is 5.51 x 102 lb?
0.348 cm3/penny
500
Titanium has five common isotopes: 46Ti (8.0%), 47Ti (7.8%), 48Ti (73.4%), 49Ti (5.5%), 50 Ti (5.3%). What is the average atomic mass of titanium?
Calculate out
500
Define Dalton’s Law of Multiple Proportions?
Elements combine to form compounds in small whole number ratios. Examples include NO, NO2, N2O, NaCl, CaF2etc.
500
Explain the difference between a molecular and an empirical formula. Can the molecular and empirical formula ever be the same.
Molecular formulas tell you how many atoms of each element are in a compound, and empirical formulas tell you the simplest or most reduced ratio of elements in a compound. They can be the same at times.
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