Science Flashcards
Does not donate all of its protons or disassociate completely.
Weak Acids
Ionize completely Hydrochloric Hydriodic Hydrobromic Perchloric Nitric Sulfuric
Strong Acids
Stronger than 100% sulfuric acid
Fluoroantimonic, Magic, perchloric acids
Superacids
When they are dissolved in aqueous solutions they conduct electricity, change blue litmus paper to red, have a sour taste, react with bases to neutralize them, and react with active metals to free hydrogen.
Acids
Pickling, remove rust and corrosion from metals. Used as catalysts in the process of minerals and the production of salts and fertilizers. Phosphoric acid is added to sodas and other acids are added to foods as preservatives or to add taste.
Uses of Acids
Measurement of the concentration of hydrogen ions in a substance in terms of the number of miles of H+ per liter of solution.
Low pH indicates a higher H+ concentration
High pH indicates a lower H+ concentration
Potential of Hydrogen pH
Pure water
pH of 7
Neutral pH
Anything with a pH lower than water (7)
Urine, stomach acid, citric acid, vinegar, hydrochloric acid, and battery acid
Acidic
Anything with a pH higher than water (7)
Drain cleaner, soap, baking soda, ammonia, egg whites, and sea water
Base
Gas molecules are small compared to the distances between them and that they are in constant random motion.
Their kinetic energy does not change with time as long as the temperature remains the same.
Higher the temperature, the greater the motion.
Kinetic Theory of gases
Derived from the kinetic theory of gases
Ideal Gas Law
The main trait of Inorganic compounds is that they lack…
Carbon
Examples include: mineral salts, metals, alloys, phosphorus and metal complexes
High melting point
Inorganic Compounds
Weaker than covalent and ionic bonds, and refer to the type of attraction in an electronegative atom. They can form within a single molecule or between molecules.
Hydrogen bonds
A molecule that is partially positively charged on one end and partially negatively charged on the other.
Polar
When the number of electrons is reduced
Oxidized
Two main characteristics are that they include carbon and are formed by covalent bonds.
Melt at temperatures below 300
Organic Compounds
Generalized principles dealing with energy and heat
Laws of thermodynamics
Two objects in thermodynamic equilibrium with the third object are also in equilibrium with each other. Being in thermodynamic equilibrium basically means that different objects are at the same temperature.
Zeroth law
Deals with conservation of energy. It states that neither mass nor energy can be destroyed; only converted from one form to another.
First law
States that the entropy (the amount of energy in a system that is no longer available for work or the amount of disorder in a system) of an isolated system can only increase. It also states that heat is not transferred from a lower-temperature system to a higher-temperature one unless additional work is done.
Second law
State that as temperature approaches absolute zero, entrophy approached a constate minimum. It also states that a system cannot be cooled to absolute zero.
Third law
Energy transfer from one body or system to another due to thermal contact
Heat
Measurement of an object’s stored heat energy and is the average kinetic energy of an object’s particles. When the temperature of an object increases and its atoms move faster, kinetic energy also increases.
Temperature
Measure of the amount of substance in an object
Mass
Measure of the gravitational pull of Earth on an object
Weight
Measure of the amount of space occupied.
Volume
Measure of the amount of mass per unit volume.
D=m/V
Density
Measure of the ratio of a substance’s density compared to the density of water
Specific Gravity
Energy transferred to a body by a means other than work.
Thermal contact
