Chapter 1 Lecture Flashcards
Study of matter—its composition, properties, and transformations.
Chemistry
Anything that has mass and takes up volume
Matter
Cotton, sand, digoxin: a cardiac drug
Naturally occurring matter
Nylon, Styrofoam, ibuprofen
Synthetic (human-made) matter
Has a definite volume, maintains its shape regardless of its container, and has particles that lie close together in a regular three-dimensional array.
Solid
Has definite volume, takes the shape of its container, and has particles that are close together, but they can randomly move around, sliding past one another.
Liquid
Usually refers to pure compounds or simple mixtures of pure compounds
Liquid
A complex liquid
Blood
Has no definite shape or volume, expands to fill the volume and assumes the shape of whatever container it is put in, and has particles that are very far apart and move around randomly.
Gas
Minimal Attractive Forces between atoms of molecules
Gas
Can be observed or measured without changing the composition of the material
Physical Properties
boiling point (bp), melting point (mp), solubility, color, odor
Physical properties
Alters the material without changing its composition
Physical change
Melting ice (solid water) to form liquid water or boiling liquid water to form steam (gaseous water).
Physical change example
Determine how a substance can be converted into another substance.
Chemical properties
Or chemical reaction, converts one substance into another.
Chemical change
A piece of paper burning, metabolizing an apple for energy, or oxygen and hydrogen combining to form water.
Chemical change examples
Is composed of a single component, has a constant composition, regardless of sample size and origin of sample, and cannot be broken down to other pure substances by a physical change. Table sugar (C12H22O11) and water (H2O) are both pure substances.
Pure substance
Is composed of more than one substance, can have varying composition (any combination of solid, liquid, and gas), depending on the sample, can be separated into its components by a physical change, sugar dissolved in water = mixture
Mixture
are complex
Mixtures
A pure substance that cannot be broken down by a chemical change.
Element
A pure substance formed by chemically joining two or more elements.
Compound
is composed of a number and a unit
Every measurement
Proper aspirin dosage = 325 (what? milligrams or pounds?). A fast time for the 100-meter dash = 10.00 (seconds or days?).Numbers need units to acquire tangible meaning
Numbers need units to acquire tangible meaning
Other units are related to the base unit by a power of 10. The prefix of the unit name indicates if the unit is larger or smaller than the base unit.The Metric System of Units – Decimal based
The Metric System of Units – Decimal based
1,000 meters (m) = 1 kilometer (km)
1 m = 0.001 km
1 meter (m) = 100 centimeters (cm)
0.01 m = 1 cm
1 meter (m) = 1000 millimeters (mm)
0.001 m = 1 mm
A measure of the amount of matter in an object.
Mass
The force exerted on the object in a gravitational field. Depends on gravitational field.
Weight
1,000 liters (L) = 1 kiloliter (kL)
1 L = 0.001 kL
1 liters (L) = 1,000 milliliter (mL)
0.001 L = 1 L
Volume = Length x Width x Height
= cm x cm x cm
= cm3
mL = 1 cm3 = 1 cc
Results from counting objects or is part of a definition. 10 fingers, 10 toes
1 meter = 100 centimeters
Exact number
Results from a measurement or observation and contains some uncertainty. 15.3 cm, 1000.8 g, 0.0034 mL
Inexact number
All the digits in a measured number including one estimated digit.
Significant figures
Are always significant
Nonzero digits
A zero counts as a significant figure when it occurs
Rules to Determine When a Zero is a Significant Figure
A zero counts as a significant figure when it occurs
between two nonzero digits, as in or at the end of a number with a decimal place.
A zero does not count as a significant figure when it occurs
Rules to Determine When a Zerois a Significant Figure
A zero does not count as a significant figure when it occurs
at the beginning of a number, at the end of a number that does not have a decimal.
Changing the position of a decimal does not change the number of significant figures.
Significant figures
The answer has the same number of significant figures
as the original number with the fewest significant figures.
Significant Figures Rules for Multiplication and Division
If the first digit to be dropped is between 0 and 4, between 5 and 9.
Then, drop it and all remaining digits, round up the last digit to be retained by adding 1.
Significant Figures Rules for Addition and Subtraction
The answer has the same number of decimal places as the original number with the fewest decimal places.
A term that converts a quantity in one unit to a quantity in another unit. They are usually written as equalities, but to use them they must be written as fractions
Conversion factor
Uses conversion factors to convert a quantity in one unit to a quantity in another unit. The units are treated like numbers and cancel any unwanted numbers.
Factor-label method
Using Conversion Factors Solving a Problem Using Two or MoreConversion Factors
Always arrange the factors so that the denominator in
one term cancels the numerator in the preceding term.
measure of how hot or cold an object is
Temperature
degrees Fahrenheit (°F), degrees Celsius (°C), Kelvin (K)
Three temperature scales are used
a physical property that relates the mass of a substance to its volume.
Density
