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Worsham Chem Q1
| Question | Answer |
|---|---|
| The study of the nature of matter & the changes that matter undergoes. | Chemistry |
| Matter | Anything that possesses mass & occupies space. |
| Nature of matter | 1) composition of a particular kind of matter 2) forces holding its parts together 3) Its observable properties |
| What are the two types of chemical bonds? | 1) Ionic bonds 2) Covalent bonds |
| What is a physical change? | A change that does not cause a change in the chemical composition of a material. |
| Melting ice, Boiling water, and Freezing water are examples of... | Physcial change |
| What is a chemical change? | A change that results in the formation of a new substance. |
| Decomp. of proteins, Cremation, and embalming are examples of... | Chemical change |
| What is energy? | The ability of a system or material to do work. |
| Kinetic energy is | energy in motion |
| Falling water, falling objects, flowing electricity are examples of... | Kinetic energy |
| Potenial energy is | stored energy |
| Stored chemical energy in food, a battery, a drawn bow are examples of... | Potenial energy |
| Inorganic chemistry is | the study of compounds USUALLY containing elements other than carbon. |
| The 4 primary classes of compounds are... | acids, bases, salts, and oxides |
| Organic chemistry is... | The study of certain carbon compounds |
| Biochemistry is... | The study of compounds produced by living organisms. |
| Proteins, carbs, and lipids are the 3 primary compounds studied in... | Biochemistry |
| Embalming chemistry is... | The study of those types of matter and changes in matter related to the disinfection & preservation of human remains. Certian aspects of all three of the major divisions of chemistry are incorporated. |
| The study of those physical & chemical changes in the human body that are caused by the process of death. | Thanatochemistry (tha-nat-o-chemistry) |
| What are the common set of units used by all scientists? | International System of Units or SI Unit or the Metric System |
| The standard unit of length is | the meter |
| The symbol for the meter is | m |
| 1 meter is equal to | 39.37" |
| The standard unit of volume is | liter |
| The symbol for the liter is | L |
| 1 liter is equal to | 1.06 quarts |
| The standard unit of mass is | kilogram |
| The symbol for the kilogram | kg |
| 454 grams are equal to | 1lb. |
| The standard unit of heat is | calorie |
| The symbol for the calorie is | cal |
| The amount of heat required to raise the temperature of 1g of water 1 degree c at 15 degrees c. | calorie |
| Calorie=kilocalorie | 1kcal=1000cal=1Cal |
| A calorie is too small a unit so a ______ is used | kilocalorie (Cal) |
| M is the symbol for... | Mega |
| The exponential expression for Mega is | 10 to the 6th power |
| k or K is the symbol for... | Kilo |
| The exponential expression for Kilo is | 10 to the 3rd power |
| d is the symbol for... | deci |
| The exponential expression for deci is | 10 to the -1 power |
| c is the symbol for... | Centi |
| The exponential expression for Centi is | 10 to the -2 power |
| m is the symbol for... | Milli |
| The exponential expression for Milli is | 10 to the -3 power |
| u is the symbol for... | Micro |
| The exponential expression for Micro is | 10 to the -6 power |
| n is the symbol for... | Nano |
| The exponential expression for Nano is | 10 to the -9 power |
| The law of conservation of mass states... | Matter is neither created nor destroyed |
| The law of conservation of energy states... | Energy is neither created nor destroyed |
| The law of conservation of energy and the 1st law of thermodynamics are the same, T/F | True |
| physical property | a characteristic that can be observed w/out altering the chemical composition of a substance |
| color, odor, taste and feel are examples of | physical properties |
| 3 typical states of matter | solid, liquid and gas |
| melting point | the temperature at which a substance changes from the solid state to the liquid state |
| the temperature at which a substance changes from a liquid to a solid | freezing point |
| the temperature at which a substance changes from a liquid to a gas | boiling point |
| solubility | the measure of how well 2 substances mix |
| the relationship between an object's mass and volume occupied by that mass | Density |
| What is the equation for density | d=m/v |
| Specific gravity | the ratio of the mass of the substance to the mass of equal volume of water at the same temp |
| What units are used in specific gravity | none. because it is a ratio of 2 masses |
| Chemical property | characteristic that can be observed when the substance is interacting with other forms of matter the interaction results in an alteration of the chemical composition of the substance |
| examples for chemical properties are | burning=match+oxygen; sodium+water=hydorgen gas & sodium hydroxide |
| Physical change | a process that manifests a physical propery |
| Chemical change | a process that manifests a chemical property. Forms new substances with their own chemical & physical properties |
| what are the stages of matter? | solid, liquid and gas |
| heat of fusion | specific quantity of heat that is absorbed to convert 1 gram of solid to 1 of liquid at the substances melting point |
| how much heat is required to change 1 gram of ice to 1 gram of water? | 80 calories |
| heat of vaporization | amount of heat needed to change 1 gram of a substance from the liquid to the gaseous state at the boiling point |
| how much heat is required to change 1 gram of water to water vapor | 540 calories |
| exothermic | the process of releasing heat |
| endothermic | the process of absorbing heat |
| sublimation | change in state directly from solid to gas |
| entropy | measure of the amount of disorder or randomness |
| plaster of Paris is an example of | exothermic |
| dry ice and heating iodine crystals are examples of | sublimation |
| which state has the most entropy | gas |
| which state has the lease entropy | solid |
| what are the properties of gases | compressibility, expansivity and diffusibility |
| no fixed volume but occupies the entire space of the container, this decribes what | the volume of a gas |
| pressure | force per unit area |
| 1 atmoshpere is equal to | 760mm Hg or 760 torr |
| what is the purpose of the gas laws | describe the relationship between a gases perssure, volume and temperature |
| Boyle's Law | relationship between the volume of a quantity of gas and its pressure when the temperature is constant. |
| the relationship between volume and pressure is _____ in Boyle's law | inversely proportional |
| breathing is an example of | Boyle's Law |
| Charles' Law | relationship between a gases volume and temperature when the pressure is constant |
| the ______ scale is used in Charles' Law | Kelvin scale |
| the relationship between volume and temperature is _______ in Charles' Law | directly proportional |
| an incubator is an example of | Charles' Law |
| the Kelvin scale is also known as | the absolute temperature scale |
| degree Celsius + 273 = | Kelvin |
| what are the properties of liquids | takes shape of the container it is in, maintians its own volume, practically incompressible, evaporation, and equilibrium |
| evaporation | transition from liquid to gas (endothermic) |
| equilibrium | when 2 opposing rates are equal |
| equilibrium vapor pressure | the pressure exerted by a vapor when it is in equilibrium with its liquid |
| as temperature increases | vapor pressure increases, therefore they are directly proportional |
| boiling | rapid passage of liquid particles to the vapor state by forming bubbles |
| normal boiling point | the BP at 1 atmosphere pressure, 760mm Hg or 760 torr |
| what is the BP of water on all three scales | 100 degrees Celsius, 212 degrees F, 373K |
| what if the FP of water on all three scales | 0 degrees Celsius, 32 degrees F, 273K |
| properties of solids | particles are held tightly together, deginate shape & volume, nearly incompressible, nearly no expansivity, low entropy. |
| melting | when heat is added to a solid, kinetic energy of the particles increases until the solid breaks apart |
| heat of fusion | the amount of heat that is absorbed to convert 1 gram of solid to 1 gram of liquid at the MP |
| matter can be divided into | pure substances and mixtures |
| pure substances are classifed as | elements and compounds |
| elements | simple substances that cannot be decomposed by ordinary chemical means |
| oxygen is an | element |
| water is a | compound |
| a mixture is | 2 or more substances not chemically united |
| mixtures are classified as | homogens and heterogenis |
| homogens | true solutions |
| heterogenis | no uniform composition |
| properties of compounds | elements join together chemically in a definate proportion by mass, can be decomposed by chemical changes |
| Law of Definite Proportions | states that when 2 or more elements combine, they will always be in a fixed or definite proportion by mass |
| what are the 4 types of compounds most important to us in inorganic chemistry | acids, oxides, salts, bases |
| properties of mixtures | formed with varying proportions of their components, can be separated by physical changes |
| an example of a homogeneous mixture is | arterial solution |
| an example of a heterogeneous mixture | sand and iron filings |
| the Law of Conservation of Mass states | matter is niether created nor destroyed |
| the Law of Conservation of Energy states | energy is niether created nor destroyed |
| the Law of Conservation of Energy is also known as | 1st Law of Thermodynamics |
| hydrolosis | water breaking down |
| proteins break down into | amino acids |
| amino acids break down into | amines and organic acids |
| amines break down into | ammonia and hydrogen gas |
| organic acids break down into | carbon dioxide, water & oxygen |
| H | hydorgen |
| He | helium |
| Li | lithium |
| Be | beryllium |
| B | boron |
| C | carbon |
| N | nitrogen |
| O | oxygen |
| F | fluorine |
| Ne | neon |
| Mg | magnesium |
| Al | aluminum |
| Si | silicon |
| P | phosphorous |
| S | sulfur |
| Cl | chlorine |
| Ar | argon |
| K | potassium |
| Ca | calcium |
| Fe | iron |
| Cu | cooper |
| Zn | zinc |
| As | arsenic |
| Br | bromine |
| Ag | silver |
| I | iodine |
| Au | gold |
| Hg | mercury |
| Pb | lead |
| What does amu stand for | atomic mass unit |
| what charge does an electron have | negitive |
| what charge does a proton have | positive |
| what charge does a neutron have | neutral |
| what particales are located in the nucleus | neutrons and protons |
| what is the name of group 1A | alkali metals or reactive metals |
| what is the name of group IIA | alkaline Earth metals |
| what is the name of group IIIA | Boron Group |
| what is the name of group IVA | Carbon Group |
| what is the name of group VA | Nitrogen Group |
| what is teh name of group VIA | Oxygen Group |
| what is the name of group VIIA | Halogen Group (salt forming) |
| what is the name of group VIIIA | noble gases or inert gases |
| which group is non-reactive and the most stabile | group VIIIA the noble gases/inert gases |
| group A elements are also known as | representative elements |
| what do the periods represent | the number of energy levels an atom has |
| what do the group numbers represent | the number of electrons in the outer most energy level |
| where is the atomic number located on the periodic table of elements | above the symbol |
| where is the atomic mass located on the periodic table of elements | under the symbol |
| how do you know how many protons an element has | the atomic number |
| how do you know how many electrons an element has | the atomic number |
| how do you know how many neutrons an element has | round the atomic mass to the nearest whole number, the atomic mass-the atomic number=number of neutrons |
| what is the equation that will tell you many electrons are in an energy level | 2n to the second power (2, 8, 18, 32) |
| how do you find the valence electron | the group number |
| how is the atomic number symbolized | the letter z |
| how are the estimated paths of electrons labeled | s, p, d, f |
| the total electrons in the outermost energy level is the | valence electrons |
| how many types does an s-orbital have, what is the max electrons that can be held | 1 type with a max of 2 |
| how many types does a p-orbital have, what is the max electrons that can be held | 3 types with a max of 6 |
| how many types does a d-orbital have, what is the max electrons that can be held | 5 types with a max of 10 |
| how many types does a f-orbital have, what is the max electrons that can be held | 7 types with a max of 14 |
| the first energy level has what orbital | only one s-orbital |
| every energy level has one ____ | s-orbital |
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