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85 Cards in this Set
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Dalton
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(1766-1844)Hypothesized that for every chemical element there is a corresponding species of objects called atoms. this atom cannot be broken down any more.
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Molecule
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Any cluster of atoms that can be isolated
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electrolysis
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"splitting by electricity" allowed for rapid discovery of many elements.
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earth's composition
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99% made of six elements: oxygen, silicon, magnesium, iron, aluminum, and calcium
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Rutherford's model of the atom
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a dense positively charged nucleus surrounded by oribiting cloud of negatively charged electrons
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other discoveries
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for each proton in nucleus there is an electron in orb it thus electrical charges of an atom cancel out and the intact atom is neutral;
if an atom should gain or lose an electron this affects its overall charge; charged atoms are called ions. |
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ground state of atoms
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all electrons in lower energy level.
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excited state of atoms
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some or all electrons are in the highest energy levels
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photon
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in bohr model when an electron drops an energy level it emits energy(visible light)
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quantam leap
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an electron must disappear and reappear on another level without transversing the distance and with no time distance
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stars
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made mainly of two elements: hydrogen and helium
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living organisms
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90% hydrogen carbon nitrogen oxygen phosphorus sulfur
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Thompson
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identified a subatomic particle called the electron, negatively charged
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Rutherford
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experimented with gold foil, proved existence of the nucleus
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electromagnetic radiation
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electrons don't fall into the nucleus
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Bohr
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said that electrons exist in various levels or shells located about the nucleus each shell corresponds to an energy level of the electron
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spectrum
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total collection of photons omitted by a given atom therefore each has a unique spectrum.
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emmission and absorption
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each element will emit and absorb light of the same wavelenght transparent or feflecting materials absorb specific wavelengths of light according to their atomic structure.
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spectroscopy
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study of elemental composition of materials by looking at absorption lines
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helium
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the elusive element, first found in suns light but not found on earth until 30 years later.
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laser
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light amplification by stimulated emission of radiation
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periodic table of elements
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elements arranged by their chemical properties.
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atomic number
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defines the sequence of elements in the table; number of protons in nucleus
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alkali metals
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first column- for example K,-Na)
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alkali earth metals
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second column (Mg, Ca)
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noble gases
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elements of the 8th column that do not form compounds readily
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atomic interaction
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explained by periodic table and bohr; when two atoms interact their outermost shell electrons dictate their interatctions and thus govern their bonding properties.
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metals
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most of the table is metals, conducts electricity well
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pauli exclusion principle
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no two electrons can occupy the same energy state(level and position in that level) at the same time.
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structure of electron shells
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there are naturally occurring spaces in the electron shells that can be filled by electrons as determined by spacing and electron spin
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shells
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1st-2 spaces
2nd shell-8 spaces 3rd shell-8 spaces 4th- 18 spaces 5th-18 spaces 6th-32 spaces 7th(highest)-32 |
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rows
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1-2 spaces
2-8 spaces 3-8 spaces 4-18 spaces 5-18 spaces 6-32 spaces 7-32 spaces |
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atomic mass
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(atomic mass)=mp+mn
mass of atom is found by adding mass of each proton and each neutron present in the nucleus. |
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electrons in outer shell
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valence electrons
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chemical bonding
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commonly involves exchange or sharing of valence electrons
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valence-
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number of elctrons in the outer shell; also the combining power of atoms
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inert gases
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(noble gas) most stable arrangement of lowest energy because all shells are filled with electrons.
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quest of the atom
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to achieve the lowest energy state it can; so when atoms come near each other they may exchange or share electrons to achieve this state.
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chemical bond
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the result of redistribution of electrons that leads to a more stable configuration between two or more atoms
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strategies of atoms
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give up electrons
gain electrons share electrons |
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result of bonding
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spontaneous- a release of energy
due to outside energy-may release or absorb energy |
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Atoms that are close to noble
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1 less- H, F, Cl
1 more- Li, Na, K, Rb tend to form ionic bonds |
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mettalic bonds
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bonds between metals; atoms float in a sea of electrons, many highly compressed gases can act as metal(O),
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alloy
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two or more metallic elements combined in a metalic bond.
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malleability
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a property of metals that allows atoms to rearrange themselves within the metallic bond to order to attain a new configuration in response to stresses; metals can be bent, shaped, molded due to this property.
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covalent bonds
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molecules that share electrons
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single bond
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one electron from each atom is shared
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the carbon bond
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the basic bond of all essential of molecules of life on earth. C atom config means it is equally likely to gain or lose 4 electrons
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the carbon-carbon system
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lower energy results from sharing of outer electrons with up to 4 other C atoms.
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organic chem
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study of C bonding and related bonding
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long chains of C and other atoms
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proteins, DNA, fats, cholesterol, etc.
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polar molecules
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molecules with either a positive or a negative side to them
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polarization
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electrons of neighbor atoms or molecules tend to be pushed away from a positive side of water; polarization makes substances like water act as a solvent(materials more easily disolves
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hydrogen bonds
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weak electrical attraction developed by the H atom itself after it is bonded to another element, like O or N
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Source of the force
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all charged parts of an atom exert electrical forces on all other neighbor atoms, so even if all atoms in a substance are electrically neutral and or non polar, the sum of the electrical charges within all atoms.
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gases
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collections of atoms or molecules that expands to take shape of and fill the volume available in a container
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atomic movement
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random bouncing off one another
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plasmas
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seas of electrically charged particles, properties can be confined by a magnetic field; conducts electricity; can grade into a gaseous state.
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liquids
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collections of atoms or molecules that have no fixed shape but maintain volume.
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water
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most common liquid on earth, but rare on other planets as far as we know.
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solids
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all materials that possess a more or less fixed ahpe and volume
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crystals
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groups of atoms that occur in a regularly repeating sequence farming a structure in which atoms or molecules occur in a regular and predictable way.
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unit cell
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the smallest subdivision of a crystal that shows the complete repeating pattern of atoms within the crystal.
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crystalline solids
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composed of interlocking crystals
natural: rocks(such as granite) man-made- alloys and ceramics organic: teeth, bones |
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glass
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groups of atoms that are may be regular on a local scale, but are not regularly distributed throughout the solid.
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polymers
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long and large molecules that are formed from numerous smaller molecules; regular pattern of atoms in one direction
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plastics
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made of intertwined polymers derived from petroleum
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liquid crystals
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an odd intermediate state of matter that is half way between liquid and crystalline solid- man made
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changes of state in matter
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freezing and melting- changes between liquid and solid
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boiling and condensation
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changes between liquid and gas
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sublimation
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change from solid to gas
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driving force: temp
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transitions result from temp changes
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chemical reactions
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atoms and molecules coming together to form larger structure or larger structures breaking apart
reactants goes to products |
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exothermic
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reactions that give off energy wile it occurs. when atoms or molecules combine the total energy is less, heat or light is given off
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endothermic
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reactions that take in energy while it occurs; when atoms or molecules combine the total energy is more so energy is absorbed
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oxidation
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giving up e- to oxygen
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combustion
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rapid oxidation reaction
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reduction
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chemical reaction in which electrons are transferred to an atom from other elements
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smelting
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reducting iron by heating in the presence of CO to make
F +CO2 |
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precipitation
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solids forming as a liquid evaporates or due to saturation in the liquid by a dissolved compound
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solution
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dissolving of solids into a liquid to dispered ions in a solution
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acid
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any material that when put in water produces positivly charged H ions in the solution
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base
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any material that when put in water produces negatively charged OH- ions
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acid-based reaction
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when two are brought together, water is formed
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acid and base with pH
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below 7 on ph scale base is above 7
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