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ch 1-4 chem
review
| Term | Definition |
|---|---|
| matter | Anything that has mass and takes up volume |
| composition | simple components that make up a material ( |
| structure | both composition and arrangement of simpler matter |
| atom | the fundamental unit of all matter |
| element | simplest form of matter and is only made up of one atom. |
| compound | composed of one or more elements in a fixed ratio and is in a fixed ratio as in you cant change it. |
| molecule | groups of atoms bound tightly together that behave as a single unit. |
| pure substance | materials only composed of one element or one compound |
| mixture | contains more than one substance and not in a bound ratio |
| homogeneous mixture | components evenly blended |
| heterogenous mixture | contain regions of significantly different concentrations |
| can mixtures be separated into individual components without changing the identity of substances? | yes |
| can compounds be separated into individual components without changing the identity of substances? | no bc it will change what it is originally |
| definite shape and volume | solid |
| no definite shape but definite volume | water |
| no definite shape and volume | gas |
| particle arrangement | the behavior of any substance is determined by the arrangement of the particles that compose the substance. |
| composes of mass, volume, temperature, color, hardness | physical properties |
| physical property | can be measured without changing the identity of the substance |
| chemical property | cannot be measured without changing the identity of substance/a change that forms new compounds |
| toxicity, acidity/basicity, reactivity, oxidation state | chemical properties |
| energy | the ability to do work |
| potential energy | energy that is stored |
| kinetic energy | the energy of motion |
| heat energy | involves the kinetic energy of the particles in a substance |
| exothermic | releases hit energy |
| hypothesis | a tentative explanation that has not been tested |
| theory | an idea supported by experimental evidence, or a paradigm, or way of thinking about a topic |
| scientific law | a statement that describes observations that are true in widely varying circumstances |
| units of measurements | quantities with accepted values that can be communicated between people |
| 10^12 1,000,000,000,000 | tera (T) |
| 10^9 1,000,000,000 | giga (G) |
| 10^6 1,000,000 | mega (M) |
| 10^3 1,000 | kilo (k) |
| 10^-1 1/10 | deci (d) |
| 10^-2 1/100 | centi (c) |
| 10^-3 1/1,000 | milli (m) |
| 10^-6 1/1,000,000 | micro (μ) |
| 10^-9 1/1,000,000,000 | nano (n) |
| 10^-12 1/1,000,000,000,000 | pico (p) |
| accuracy | how reliable are the measurements are |
| precise | how closely grouped together they are |
| significant digits | indicate how precisely we know a measurement and they show the precision of a measured quantity |
| 1. all nonzero digits are significant, and all zeros between nonzero digits are significant 2. if a decimal point is present, zeros to the right of the last nonzero digit are significant 3. zeros to the left of | significant digits |
| exact numbers | values for which there is no uncertainty |
| circumference of a ball | c=πd |
| volume formula | mass x length x height |
| d = m/v | density formula |
| v = m/d | if density is given but not volume |
| m = v x d | if density is given but not mass |
| water's density | 1.00 |
| F = 9/5°C + 32 | farenheit conversion |
| C = 5/9(°F −32) | celsius conversion |
| K = °C + 273.15 | kelvin conversion |
| law of conversation of mass | in chemical reactions, matter is neither created or destroyed (Antoine Lavoisier) |
| atomic theory | •Elements are made of tiny, indivisible particles called atoms • The atoms of each element are unique. • Atoms can join together in whole-number ratios to form compounds. • Atoms are unchanged in chemical reactions. |
| periodic table of elements | Arranged by atomic mass and properties (Mendeleev) |
| groups | columns in the periodic table (have similar properties) |
| periods | rows in the periodic table |
| metals | to the left of the periodic table |
| non-metals | to the right of the periodic table (the building blocks of life) |
| metalloids | located in between metals and nonmetals (semiconductors) |
| alkali metals | soft metals that react violently with water group 1 |
| alkaline earth metals | less reactive than group 1 (burns brightly) group 2 |
| halogens | diatomic molecules in an element form many different compounds group 7 |
| noble gases | generally do not form compounds and are gases at room temperature group 8 |
| subatomic particles | particles that make up atoms |
| 1 u = 1.66 × 10^−27 kg | atomic mass unit |
| opposite attracts and like charges repel | charges |
| electrical energy | a form of energy that involves the motion of charged particles. |
| electron | a tiny, negatively-charged particle mass of each particle is 1/2000 the mass of a hydrogen atom. |
| ernest rutherford and his model | Positive charge is localized over a very tiny volume of the atom, which also contains most of the atom's mass |
| plum pudding model | envisioned negative electrons spread throughout a positively-charged material. |
| alessandro volta | invents electrochemical cell (battery) Flow of charged particles generates electrical current |
| atomic number | number of protons and also the number of electrons in a neutral atom |
| atomic identity | the number of protons determines the identity of the atom |
| mass number | p+n |
| isotopes | have the same atomic number, but different mass number |
| average atomic mass | a weighted average of the different isotopes of an element. |
| average value | average value = (value A × fraction A) + (value B × fraction B) |
| bohr model | electrons orbit the nucleus. • Only certain orbit energies are “allowed”. • Electrons can jump between levels. • Light is absorbed or released when electrons jump. |
| quantam model | electrons behave as particles and waves |
| ions | an atom or group of atoms with an overall charge |
| light | electromagnetic radiation • a form of energy • travels in waves • exists in increments called photons |
| electromagnetic spectrum | tv/radio - lowest frequency and wave (0) microwave infrared (600) visible UV (500) x rays (400) gamma rays |
| wavelength | the length of one wave |
| frequency | the number of waves per second |
| speed of light formula | c = wavelength x frequency |
| 3.00 × 10^8 m/s | speed of light |
| red wave length | longer wavelength lower frequency lower energy |
| blue wavelength | shorter wavelength higher frequency higher energy |
| E = hv (v is frequency and h is plancks constant) or E=hc/wavelength | energy of photon |
| line spectra model | white light is composed of all colors of light Light from a heated hydrogen gas only produces only specific colors |
| line spectra | each element produces a unique line spectrum. this is the fingerprint of each element. |
| photoelectric effect | light causes atoms to eject electrons and that there is a dense nucleus |
| heisenberg’s Uncertainty Principle | It is impossible to precisely know the exact velocity and location of a particle. |
| capacity of 2 electrons | energy level 1 |
| capacity of 8 electrons | energy level 2 how many electrons? |
| capacity of 18 electrons (levels) | energy level 3 how many electrons can it hold? |
| energy level 4 | capacity of 32 |
| 1 orbital | sublevel s how many orbitals? |
| 3 orbitals | sublevel p how many orbitals? |
| 5 orbitals | sublevel d how many orbitals? |
| 7 orbitals | sublevel f how many orbitals? |
| orbital | are the region where the electrons are most likely to be found |
| 2 | how many electrons can a orbital hold? |
| 2 | how many electrons in sublevel s |
| 6 | how many electrons in sublevel p |
| 10 | how many electrons in sublevel d |
| 14 | how many electrons in sublevel f |
| hund's rule | if empty orbitals of the same energy are available, electrons singly occupy orbitals rather than pairing together. |
| isoelectronic | have the same electron configuration |
| valence electrons | electrons in the highest occupied energy level (s and p levels) |
| other electrons | electrons beyond the largest FILLED noble gas |
| inner electrons | non bonding electrons |
| octet rule | an atom is stabilized by having its highest-occupied (valence) energy level filled. |
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