Chemistry Study for Test 1 PDF

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Chemistry Study for Test 1 (Prep study abeka)...

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Chemistry Study Preparation for Test 1 Notes Chemistry the branch of science that deals with the study of composition, structure, and properties of matter and the changes that matter undergoes Physical chemistry the foundational to the other areas of chemistry, deals with applying the theories of physics to the study of reaction properties of matter. Organic chemistry study substance that are compounds of carbon inorganic chemistry generally deal with substances that are chemical combinations of elements other than carbon Biochemistry the chemistry of living things analytical chemistry deals with identifying what substances are present in material and how much of each substance is presence sciencethe systematic study of God's universe and how it works scientific method to guide man's study of creation; consists of observing, hypothesizing, and experimenting. Observing gathering data hypothesizing suggesting explanation for observation experimenting setting up carefully controlled artificial situations theory once a hypothesis has been support by many many experiment and verified by other scientists it is considered scientific law a theory that has stood the test of time may be mathematics the language of science Precision has to do with the consistency of reproducible of a measurement and is closely related to a measurement's uncertainty Accuracy has to do with how close a measurement is to the actual, exact value exact numbers values obtained by counting or set by a definition system of measurmentis a collection of compatible, related units that can be used to measure carious quantities. metric system a worldwide as the standard of measurement SI this system often called is a modification of the metric system with meticulously defined standard for all units prefixes to the base unit's name to change its value meter the standard SI unit of length nano n, one billionth 10 ^-9 micro μ, one millionth 10^-6 milli m one thousandth, 10^-3 centi c, one hundredth 10 ^-2 kilo k, one thousand 10 ^3 mega M, one million 10^6

Liter defined as 1000 cubits centimeters, or approx. the volume of cube 4 inches mass the quantity of matter in an object weight the force of gravity upon an object kilogram is more commonly used in everyday measurements and is the unit defined by the SI Density represented by the lowercase ρ, it measures the compactness of matter. ρ= m/v degrees Celsius in Chemistry, temperature is most often measured absolute zero the coldest possible temperature kelvin is the same size as a degree Celsius, but the scale assigns that value 0 K to absolute zero ( t c= T k - 273.15 second unit of time dimensional analysis the value is multiplied by a conversion factor, a fraction that equals one and has different units in the numerator and denominator scientific notation based on the fact that every number can be expressed as a number between 1 and 10 multiplied by a power of 10 significant figures the digits that are certain along with the one uncertain digit matter often defined as anything that occupies space and mass kinetic energy the energy of motion solid characterized by a definite shape and volume melting point the substance reaches a certain temperature called..... liquid the particles have enough kinetic energy to break loose from their rigid position boiling point the particles gain enough kinetic energy to break away gas doesn't have a definite shape or volume plama a hot gas which atoms are broken down to form charged particles or ions substance a form of matter with unique properties that make it different from other substance atoms small particles elements substances such as copper, cannot be broken down into simpler substances by ordinary chemical means molecules groups of two or more atoms that are linked by a chemical bond to form distinct units. Atomic symbol each element has an compounds a substance such as water that can be decomposed by chemical means into simpler substances formula a grouping of symbols that tells what types of atoms compose the compounds and the number of each type of atom in each molecule. pure substances both elements and compounds can be described as.... homogeneous they are composed of the same kind of matter throughout a sample mixture a substance consisting of two or more pure substances that are physically mixed by not chemically combined heterogenous mixture consists of pure substances that are incompletely mixed. phase a homogeneous part of a system that is in contact with but physically distinct from other parts of the system. atomic theory This theory states that: 1. every element consists of tiny indivisible, indestructible particles called atoms,

2. all the atoms of particular element have the same size, mass, and chemical behavior 3. Differences in the properties of elements, result from differences in the atoms of the elements 4. the atoms of elements combined in a compound are combined are combined in a definite ratio 5. A chemical reaction is the result of rearrangement, combination, or separation of atoms law of definite composition the first basic law explained by Dalton's theory: states that the ratios of the masses of each element in a given compound are always the same law of multiple proportions states that when two elements can combine to form more than one compound, the masses of one element that combine with a fixed amount of the other element are in a ratio of small whole numbers properties one type of matter may be described, identified, or distinguished from another by its... chemical properties other properties describe how matter reacts to change into other chemically different substances having different properties, these are called what? physical properties Properties described a substance's appearance are? e.g. color, odor, density, hardness, solubility, taste, boiling point, and melting point physical changes Changes in the physical appearance of matter that do not change the identity or chemical composition of a substance (physical changes may be reversed physical process) chemical change A change in which a substance becomes a different substance with a different composition and properties (chemical changes can be reversed only by chemical changes) distillation homogeneous mixtures (solutions in liquid form may be separated by... precipitate formation of a insoluble substance fractional crystallization a solid containing a relativity small amount of of solid impurity may sometimes be purified chromatography complex mixtures can by separated the technique subatomic particles smaller particles of matter electrons a substance known to become electrically charged when rubbed with silk cathode the charged electrical lead electrod Humphrey Davy The English chemist Michael Faraday Physicists used electrons protons positively charged particles nucleus the existence of a small, central containing virtually all of the mass planetary model also known as the nuclear, only when an ion "bullet" came near a nucleus would be repelled and deflected; most of the ions would pass through undeflected because they would encounter mostly empty space or very light electrons neutron a neutral particle atomic number atomic number is often the given the symbol Z/ All of the same elements has the same same number of protons and hence the same atomic number, z mass number the sum of the number of protons and the number of neutrons in a nucleus nucleons nuclear particles, whether neutrons or protons, are known collectively. isotopes atoms of the same elements that differ in their mass numbers are... ion atoms or molecules often have a different number of electrons than protons, anion an ion with more electrons than protons has an excess of negative charge cation a positively charged ions atomic mass John Dalton developed the concept of

atomic mass units atomic is usually measured in... mass spectrometer atomic masses can be measured with high precision using mass spectruma record of the mass distribution of particles in a sample is average atomic mass we refer to the atomic mass of an element we usually mean weighted average to determine the average atomic mass, is used to account for the natural abundances of the isotopes A=Z+N equation quark The building blocks of the atom's nucleus are actually composed of even smaller particles called...