Term
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Definition
| Chemistry is properties of matter and the changes it undergoes, + the energy changes that accompany them. |
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Term
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Definition
| Entropy is a measure of disorder; randomness. |
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Term
| Things are naturally inclined towards _____ entropy and ______ energy. |
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Definition
| Things are naturally inclined towards increasing entropy and decreasing energy. |
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Term
| Bubbles that form on in boiling or near-boiling water are made of... |
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Definition
| Bubbles that form on in boiling or near-boiling water are made of water vapor |
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Term
| How is "sweat" on the outside of a cold glass of milk formed? |
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Definition
| "sweat" on a cold glass of milk is caused by water vapor condensing from the air (since the glass is colder than the surrounding air) |
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Term
| When water evaporates, what happens to the bonds? |
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Definition
| When water evaporates, the bonds don't break; they just s p r e a d o u t |
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Term
| Forming of bonds creates.... |
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Definition
Forming of bonds creates energy.
Breaking bonds does NOT create energy. (common misconception) |
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Term
| When ice cubes in a glass of water melt, what happens to the water level? |
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Definition
| When ice cubes in a glass of water melt, the water level remains the same; the water was just displaced by the ice |
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Term
| What # is used to express the number of particles within 1 mol of a substance? |
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Definition
6.02 x 1023
the number of particles in 1 mol of a substance |
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Term
| The higher the specific heat of a subtance, the _____ it will take to heat that substance |
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Definition
| The higher the specific heat of a subtance, the longer it will take to heat that substance |
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Term
| What happens to the concentration of a salt & water solution when 1/2 of the water is evaporated? |
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Definition
| The concentration will remain the same. |
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Term
| List steps of the "scientific method" |
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Definition
1. Observation/Problem
2. Hypothesis
3. Experiment
4. Theory (explains why)
5. Law (explains what exactly happened) |
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Term
| List the 7 basic measurements of Chemistry, their symbols and what they are a unit of |
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Definition
The 7 basic measurements of Chemistry (Systeme Internationale)
invented by group of scientists after the French Revolution
1. kilogram (unit of mass) - kg
2. meter (unit of length) - m
3. second (unit of time) - s
4. Kelvin (unit of temperature) - K
5. Ampere (unit of current) - Amp. or A
6. Candela (unit of luminous intensity) - cd
7. Mole (unit of amount) - mol
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Term
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Definition
a thousand
i.e - kilometer (1000 x 1 meter) |
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Term
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Definition
10 times
10 x base unit
i.e dekameter, Dm (10 x 1 m.) |
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Term
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Definition
1/100 x base unit
ie. centimeter (100 centimeters in 1 meter) |
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Term
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Definition
1/10 x base unit
i.e decimeter - 10 decimeters in 1 meter |
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Term
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Definition
1/1000 x base unit
i.e millimeter (1000 millimeters in 1 meter) |
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Term
| How can you tell how precise something is by looking at significant figures? |
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Definition
Significant figures indicate the precision of the measuring tool, equal to number of certain digits + 1 uncertain digit.
The more significant figures, the more precise; also indicates that the measuring tool is very precise |
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Term
| Leading zeroes in a number are always... |
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Definition
Leading zeroes in a number are always insignificant/ not significant.
(i.e - 0.0014 has only 2 SFs) |
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Term
| Trailing numbers in a figure are... |
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Definition
| Trailing numbers (at the end) in a figure are only significant if there is a decimal place |
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Term
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Definition
| Captive zeroes (in between non-zero numbers) are always significant. |
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Term
Density
Definition & Formula |
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Definition
Density tells how concentrated the mass of an object is
Density = mass
_______
volume |
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Term
| Explain measuring by displacement |
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Definition
| Volume of an object can be determined by displacement. If you put water in a tube, measure the volume, then add the object to the tube, measure the volume, and determine the diffference, that will give you the volume of the object |
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Term
| What must you remember to do to the answer when dividing or multiplying two figures? |
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Definition
When you have divided or multiplied two figures that each have a different number of significant figures, round the answer to number of significant figures belonging to least precise number.
ie. D = 4.558 / 153
4.558 has 4 SFs. 153 has 3 SFs. Therefore the answer needs to be rounded to have just 3 SFs.
0.297908 |
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Term
| What must you remember to do to the answer after you have added or subtracted figures? |
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Definition
| When you add/subtract figures, round the answer to the # of decimal places of the least precise # (the number with the least amount of decimal places) |
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Term
| How do you determine the number of significant figures when looking at a number written in scientific notation? |
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Definition
In scientific notation, they are all significant figures...
For example
1.20 x 103
has 3 significant figures; even the trailing zero is counted |
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Term
| How many yards in 1 meter? |
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Definition
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Term
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Definition
| A random error or indeterminate error means that the measurement has an equal probability of being high or low |
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Term
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Definition
| Systemic Error/ Determinate Error - occurs in the same direction each time; it is either always high or always low |
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Term
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Definition
| Exact numbers are numbers that were not obtained using measuring devices, but were determined by counting - ie. 10 experiments, 3 apples, etc. |
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Term
| Temperature in K -> temp. in Celsius |
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Definition
| K - 273.15 = temp. in Celsius |
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Term
| Temperature in Celsius -> Fahrenheit |
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Definition
| 9/8 (degrees Celsius) + 32 = degrees Fahrenheit |
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