BJU Physical Science Chapter 12-21 (CCA Final Exam Review)
metaloids
"almost metal" that slightly conduct electricity
molarity
(M) Solution concentration measured in units of moles of solute per liter of solution
True
(True or False) Atomic mass did not always produce a table with similar elements next to each other.
True
(True or False) no alkali metal has been found as a pure mineral in nature.
maximum electrons per energy level
1 - 2, 2 - 8, 3 - 18, 4 - 32
S shape contains _______ orbital(s) and _______ electrons
1, 2
writing chemical formulas - rules
1. write symbols of 2 elements next to each other with less electronegative element first 2. find oxidation numbers and write above symbols 3. use subscripts to adjust the quantities of the atoms so that the sum of the oxidation numbers equals zero - may need to use LCM 4. the sum of all the atoms in a polyatomic ion is equal to its charge - put ion in parentheses when adding a subscript
atomic mass unit
1/12 the mass of a carbon-12 atom with 6 protons and 6 neutrons - represented as u - this unit is approximately equal to the mass of one proton or neutron
J.J. Thompson
1897- discovered small particles in the atom. Was the first to disprove that atoms are indivisible. Used a cathode-ray tube and electrically charged plates to realize that atoms have a negative charge. Called the small negatively charged particles in the atom corpuscles (electrons). Made the plum pudding model as a theory as to the arrangement of the electrons.
Niels Bohr
1913- discovered that electrons move around the nucleus in orbits called electron clouds - through his experiments he found 1- electrons occupy different energy levels in the atom 2- different elements give off different colors when heated 3 - each element has a unique electron structure - developed the Planetary Model of the atom
Ernest Rutherford
1919 - solar system model of the atom, gold foil experiment- fired negative ions at thin sheet of gold foil, discovered the atomic nucleus and proposed the Nuclear Model of the atom .
James Chadwick
1932 - discovered the neutron
D shape contains ________ orbital(s) and ______ electrons
5, 10
F shape contains _________ orbital(s) and _______ electrons
7, 14
physical change
A change in a substance that does not involve a change in the identity of the substance
chemical reaction
A change of composition, represented symbolically by a chemical equation.
chemical change
A change that occurs when one or more substances change into entirely new substances with different properties. *Cannot be undone by physical processes Evidence of this: 1. a solid separates from a liquid mixture of chemicals 2. a gas is produced by means other than evaporation 3. a substance's color changes and is usually permanent 4. the temperature of a substance changes 5. light, sound, or another type of energy is produced
Law of Definite Proportions
A chemical compound always contains exactly the same proportion of elements by mass - Joseph Louis Proust
empirical formula
A chemical formula that shows the smallest whole-number ratio of elements in a compound. An ionic compound's formula unit is the same as it's empirical formula. Not unique to the chemical compound to which it refers.
single-replacement reaction
A chemical reaction in which one element in a reactant compound is replaced by an element (another reactant). The replaced element is one of the products, usually forming a precipitate or a gas. Always contains at least 3 elements.
double-replacement reaction
A chemical reaction in which two ionic compounds swap cations with each other, usually forming a precipitate compound as one of the products.
composition reaction
A chemical reaction yielding a single product from several reactants. Also called synthesis reaction and combination reaction.
decomposition reaction
A chemical reaction yielding two or more products from a single reactant. It is usually an endothermic reaction.
continuous spectrum
A complete visual spectrum with no frequency gaps, emitted only by an ideal luminous object.
binary compound
A compound composed of only two different elements. Can have more than 2 atoms, but only 2 different elements.
beam
A continuous stream of photons moving in the same direction.
lens
A disk of transparent material that refracts light so that the lgith converges or diverges.
Colloidal Dispersion
A heterogeneous fluid mixture in which the particles of the dispersed phase are between 1nm and i um in diameter.
Aerosol
A heterogeneous mixture of tiny solid or liquid drops dispersed in a gas.
Emulsion
A heterogeneous mixture that contains two or more immiscible liquid phases
Suspension
A heterogeneous mixture that separates into layers overtime
Solution
A homogeneous mixture of two or more substances
Spring
A laboratory mass that is suspended from a spring which oscillates up and down.
meniscus lens
A lens that has one convex side and one concave side. It is preferred for glasses because it provides a larger area of corrected vision.
diverging lens
A lens that is thicker at its edges than at its center. It spreads light rays apart.
converging lens
A lens that is thicker at its optical center than at its edges. It focuses light rays to a point.
incident ray
A light ray approaching a reflective surface or a boundary between different refractive media.
reflected ray
A light ray moving away from the point of reflection.
charge-coupled device (CCD)
A light-sensitive, semiconducting surface used in cameras in place of photographic film.
Solvent
A liquid substance capable of dissolving other substances
inverse-square law
A mathematical relationship in which the magnitude of one quantity varies with the inverse of the square of another. It applies to many areas of physics, such as gravitational force,light illumination, electrostatic force, and electromagnetism.
optical density
A measure of a transparent material's ability to transmit light; similarly, a measure of a material's ability to absorb light.
computed axial tomography (CAT/CT)
A medical imaging technology that uses x-rays to obtain cross-sectional images or "slices" of the body, which then can be assembled by computer to produce a three-dimensional image.
Stock system
A method of naming an ionic compound to indicate the metal's oxidation number when the metal can have more than one common oxidation number - a Roman numeral in parentheses following the metal's name represents the value of the metal's oxidation number for that compound.
Supersaturated
A mixture that has more dissolved solute than is predicted by its solubility at the given temperature. Highly unstable
Conjugate acid
A new acid when acids dissolved in water
Conjungate base
A new base that is formed when a acid is dissolved in water
nuclear fission
A nuclear reaction in which a massive nucleus splits into smaller nuclei with the simultaneous release of energy - fissions cause fissions (nuclear chain reaction) - 20% of the energy in the US is produced this way
nuclear fusion
A nuclear reaction in which atomic nuclei of low atomic number fuse to form a heavier nucleus with the release of energy - produces even more energy than fission - this type of bomb can be 1000 times more powerful than a fission bomb - has been called the energy of the future - energy operations using this are scheduled to begin in France in 2021
Huygeens
A person who build a clock on Galileo's design.
Dispersed Phase
A phase that is a minority in a heterogeneous mixture and that is dispersed or suspended throughout the continuous phase
spectrograph
A photograph, printout, or other display of a spectrum produced by a spectroscope.
plane mirror
A reflective surface having no curvature; a flat mirror.
chain reaction
A series of reactions in which the product or by-product of the reaction initiates further reaction - happens in nuclear fission - see diagram on p.402
chemical formula
A shorthand way to represent the identity and the relative amounts of elements in a compound. Element symbols are used to show which elements are present. Subscripts are used to show how many atoms of each atom are present in a molecule.
Amalgam
A solution of two metals. One of which is usually mercury
Unsaturated
A solution that contains less than the maximum amount of dissolved solute in a concentration
line spectrum
A spectrographic display of lines representing electromagnetic emissions in discrete frequencies or wavelengths.
concave mirror
A specularly reflective surface shaped like the interior of a greatly flattened bowl. The surface bulges away from the object being reflected.
convex mirror
A specularly reflective surface shaped line a dome. The surface bulges toward the object being reflected.
Insoluble
A substance that does not dissolve in a solvent
Solute
A substance that is dissolved in a solution
reactant
A substance that is present before and takes part in a chemical reaction. It appears on the left of a chemical equation.
product
A substance that is produced in a chemical reaction. It appears on the right of a chemical equation.
Immiscible
A term used to describe liquids that are not able to dissolve/mix in one another
Gel
A two-phase heterogeneous mixture in which dispersed solid particles form an open network throughout a liquid continuous phase.
Sol
A two-phase heterogeneous mixture in which the dispersed solid phase does not form an open network in the liquid continuous phase as in a gel.
coefficient
A whole-number multiplier appearing in front of a chemical formula in a balanced chemical equation, indicating the proportion of each element or compound needed to ensure the conservation of mass during a chemical reaction. When no coefficient appears in front of a chemical formula, a coefficient of 1 is assumed.
Litmus paper turns Red in _____________ solutions
Acids
Neutralization
Acids and bases can cancel out each others chemical action In a reaction/ forms water and salt
Metals
All of these (except Hg) solids at room temperature.
color system
All possible colors that can be produced by the combination of a specific set of primary colors. A --- is identified by its primary colors.
plum pudding model
An early model of the atom that described it as a positively charged sphere in which negatively charged electrons were randomly scattered - developed by JJ Thomson - was not able to explain what gives atoms their mass since electrons have very little mass
chemical equation
An equation that symbolically represents the identity and amounts of reactants and products that take part in a chemical reaction.
real image
An image formed when light rays from a point on an object converge after reflecting off a mirror or passing through a lens. A -exists apart from any visual system perceiving it.It is upside down and revered and can be projected on a screen.
principal optical axis
An imaginary line normal to the optical center of a concave or convex mirror or lens. It is used as a reference when describing the characteristics of the optical device.
Litmus paper turns Blue in _____________ solutions
Bases
Soluble
Capable of being dissolved
Metals
Clean surfaces of most _______ have a silvery luster.
Acid strength
Degree of ionization
Base strength
Determined by the degree of ionization
What are naturally occurring molecules of 2 atoms?
Diatomic elements
give away because they have low EN
Do alkaline give away or take easier?
infrared
EM waves that have wavelengths longer than red light, shorter than microwaves. Is not visible, but can be felt as heat. produced by the thermal motion of atoms and molecules. (supports thermal imaging, "night vision" and digital communications.
Family
Each column on the periodic table is called a ___________.
What is the only pure substance that is made of only 1 kind of atom?
Element
Properties of acids
Form electro ties, that are ions in the solution conducts electricity
Democritus
Greek student of Leucippus who coined the word atomos or atom, meaning indivisible. He was the first person who stated that everything was made up of atoms. He did not do any experiments to test his atomic theory. His model was called the universal atomic model.
alkali metals
Group 1A metals that have One Valence electrons that can be removed easily, making these metals very reactive
alkaline-earth metals
Group 2A that has TWO valence electrons making them slightly less reactive than their "close cousins the alkali" . Found in many minerals.
carbon family
Group 4A , begins with Carbon. Includes nonmetals, metalloids and soft metals. Have 4 valence electrons
Alkali metals
Group one a is also know as the ________ ________.
transition elements
Groups 1B-8B . Metals that have similar chemical and physical properties and 1 or 2 valence electrons
ray
a. Mathematically, a line segment with an arrowhead showing direction. b. In optics, a representation of the path a light photon takes.
soluble
able to dissolve in a certain solvent
nuclear decay
alpha, beta, and gamma - occurs naturally
Which hydrogen is most easily ionized?
The first available hydrogen atom
crystal lattice
an extensive, repeating, three-dimensional arrangement of atoms or ions
photometer
an instrument that measures luminous intensity or brightness, luminous flux, light distribution, color, etc., usually by comparing the light emitted by two sources, one source having certain specified standard characteristics.
electron affinity
an unbonded atoms ability to attract and hold electrons
continuous phase
an unbroken phase that makes up most of a heterogeneous mixture in which other phases are dispersed
bioluminescence
any form of light produced by animals or plants through biological processes.
negative oxidation number
atom gains that many electrons - these atoms have high electronegativity
octet rule
atoms generally are most stable when they have a full eight electron in there valence shell
isotopes
atoms of the same element that have different numbers of neutrons - number of protons is the same
octet rule
atoms tend to gain, lose or share electrons so as to have eight electrons in their outer electron shell - all atoms do not follow this rule - the most electrons that can be in the outermost energy level is 8 and the fewest is 1
Nonmetals
Six __________ called inert or Noble gases Do not readily react with other elements.
Properties of bases
Soapy or slipperly
Nonmetals
Solid ___________exist as brittle crystals that shatter easily.
Miscible
Soluble in another liquid
Acids taste
Sour
Example of Diprotic acid
Sulphlartic h2so4
radio-frequency identification (RFID)
Technology that uses radio-frequency induction to generate an identification signal from a microprocessor receiver and antenna assembly.
television
Technology used to transmit moving images with synchronized sound using formatted radio-frequency signals; a device which reproduces video and audio televised signals.
fiber optics
Technology using bundles of long, fine, transparent glass fibers that transmit light along their lengths by total internal reflection.
critical angle of incidence
The - that produces an angel of refraction of 90 degrees for a light ray traveling from a medium with a higher index of refraction to one with a lower index; that is, the refracted light ray is parallel to the boundary surface between the media.
Saturated
being the most concentrated solution possible at a given temperature
ionic
bond between a metal and a nonmetal
metallic
bond between two metals
covalent
bond between two nonmetals
covalent
bond that shares electrons
ionic
bond that takes and gives away electrons
metallic
bond that with a sea of electrons
quantum model of the atom
early 20th century scientists discovered the electron acts like both a wave and a particle - they refined the Bohr's planetary model to reflect this - this model shows the distribution of electrons in the atom as a cloud with no clearly defined boundaries (the previous model used circular orbits) - this is the current accepted model of the atom
gamma rays
electromagnetic waves with no mass or charge
valence electrons
electrons in the highest energy level of an atom - determine important chemical properties of an element - every neutral atom has these
fluorine
element with the highest EN
nonmetals
elements that lack most of the properties of metals; reside above and to the right of the "stair step" on the periodic table
family
elements with the same # of Valence electrons often share similar physical and chemical properties
atoms which do not have eight electron (such as hydrogen and helium)
exceptions to the octet rule
halogens
family with the highest EN
Metal characteristics
few valence electrons, electrons easily lost, shiny, ductile, malleability, good conductors and very reactive
acoustic spectrum
formed by sound waves; consists of waves with differing frequencies (vibrations per second), including frequencies too low to hear, audible sounds, and frequencies too high to hear
beta particles
free nuclear electrons produced by the decay of neutrons - have little mass and a negative charge
forms of nuclear decay
gamma, alpha, beta
free or pure elements
have an oxidation number of zero
metals
have few valence electrons that are not held very strongly together. ; reside in the 2/3 of the left of the "stair step" in periodic table
illuminated object
have many different colors, and the same object can appear to have different colors under differnet color
protons and electrons
have the same magnitude of charge
monatomic
having one atom in the molecule
Aberdeen, Scotland
his first teaching position at college?
Dewar
his wife?
Non-metal characteristics
hold valence electrons tightly, mostly gas but exist in solids, poor conductors, variety of color and noble gases do not react
candela (cd)
The SI base unit of light intensity
Dissociation
The action by the solvent in breaking apart an ionic compound's crystal lattice to form a solution
Joseph Louis Proust
in 1790, this chemist discovered the Law of Definite Proportions
physics, astronomy,1871
in 1860 he became professor of-- and -- in
the law of the conservation of matter
in a chemical reaction, matter is neither created nor destroyed - the number of atoms before the reaction must equal the number of atoms present after the reaction
light dispersion
The angular separation of the various frequencies in a beam of light by refraction, as with a prism. The dispersion angle is greater for higher frequencies.
saturation
The apparent brightness, or intensity, of a color.
phosphorescence
The continuing emission of visible light after a substance has been exposed to high-frequency electromagnetic energy.
value
The darkness or lightness of a color.
Wavelength
The distance between corresponding parts of two consecutive waves. Lambda.
focal length
The distance from the center of a lens or mirror to its principal focus.
light-year (ly)
The distance light travels in one year, approximately 9.6 trillion km (6 trillion mi); the unit of distance (not time) best applied to objects far outside our solar system.
x-ray
The electromagnetic band extending from 30 PHz - 30 EHz, there is some over lap with gamma rays. They are produced by high-energy collisions of electrons with atoms.
Transition metals
The elements in the middle of the periodic table that all have one or two electrons.
fluorescence
The emission of visible light by a substance that is exposed to high-frequency electromagnetic energy.
Transverse waves
The individual particles vibrate at right angle to the direction of the wave.
Longitudinal wave
The individual particles vibrate in the same direction as the wave.
Periodic law
The law which states that the properties of elements vary in a periodic or recurring patter with their atomic mass.
Amplitude
The maximum distance from the rest position.
diffuse reflection
The most common type of reflection in which photons reflection in which photons reflect off an uneven surface in all directions. An image of the light source cannot be formed from a-----
electrolysis
The process of decomposing a chemical compound by the passage of an electric current - often done with water yielding hydrogen and oxygen gas - chemical change
intensity
The rate at which a light source radiates energy, measured in candelas (cd), which is an SI base unit. Also called brightness.
index refraction
The ratio of the speed of light in a vacuum to the speed of light in a given medium; a measure of a medium's optical density.
Henry's Law
law stating that the greater the pressure of a gas on a liquid, the greater the mass of the gas that can dissolve in the liquid at a given temperature
core-envelope model
model by John Dalton where each element has its own kind of indivisible atom and the atomic mass differences are due to the varying thickness of their "heat envelopes"
planetary model of the atom
model that shows the electrons orbiting at fixed distances (energy levels) around the nucleus - electrons cannot occupy the areas between the energy levels in this model - this model developed by Bohr looks like a miniature solar system
reverberations
multiple echoes of a sound formed when it reflects off distant surfaces; can distract or irritate listeners and cause speech and other sounds to be unintelligible
scientific models
must be workable or give useful answers to the questions scientists ask - when new information is discovered and scientist change their way of thinking, the _____________ change to reflect this
radio astronomy
The study of celestial objects by observing the radio waves they emit and the study of near-earth objects using active radar pulses.
Alchemy
The study of chemistry in attempt to cheap metals into Gold or silver.
Alkaline earth metals
These are close cousins of but much less reactive than the alkali metals.
Metaloids
These are slightly conductive thought nowhere nearly as conductive as metals.
Metals
These elements occupy about three fourths of the periodic table.
Nonmetals
These exist as Solids, Liquids, and Gasses at room temperature; most are gases.
Nonmetals
These have a variety of colors.
Metals
These tend to be reactive, easily forming bonds.
pH indicator
They change colors in the presence of acids
Semiconductors
This is one of the main uses of metalliods in computers.
Metalloid
This word means "almost metals"
Triprotic acid
Three ionizable hydrogen atoms
Johann Dobereiner
Which Chemist in 1829 Found several smell groups of elements with similar properties.
John Newlands
Which Chemist in 1866 arranged the elements in a table in order of their increasing atomic masses.
Dimitri Mendeleev
Which scientist proposed a system that organized the elements in order of increasing atomic masses, and left places for then missing elements.
left to right
Which way does EN increase on the periodic table?
Antoine Lavoisier
Who dealt a death blow to Aristotle's idea when he Broke down water into hydrogen and oxygen.
Berzelius
Who developed a system based on the first two letters of an element's Latin name.
incomplete valence energy levels
Why are some atoms unstable?
to lower energy level and to gain stability
Why do atoms bond?
Nonmetals
_________ other than the noble gasses generally form bonds by sharing or taking electrons from other atoms.
Aristotle
a Greek philosopher who rejected the teachings of Democritus and said that matter was continuous without any distinct particles - he influenced science for 2000 years
nonpolar bond
a bond between two atoms of the same nonmetal element. Electrons are evenly shared, so no partial charges exist at the ends of the bond.
electronegativity
a bonded atom's ability to attract and hold electrons
larynx
a box-like structure located at the top of the trachea; your voice box
exothermic
a chemical reaction that releases energy - this energy is listed with the products of the reaction - Q listed in the products denotes the production of thermal energy - i.e. gasoline burning in a car engine to produce the energy needed to move the car
saturation
a comparison of the concentration of a solute in a solution to its concentration at its solubility limit
polar covalent bond
a covalent bond between two elements with different electronegativities, resulting in uneven electron sharing that creates opposite partial charges at opposite ends of the bond, like electrical poles
spectroscope
a device that breaks up light into its component colors
colloid
a heterogeneous fluid mixture in which the particles of the dispersed phase are between 1 mn and 1 um in diameter
colloidal dispersion
a heterogeneous fluid mixture in which the particles of the dispersed phase are between 1 nm and 1 micrometer in diameter
suspension
a heterogeneous fluid mixture in which the particles of the dispersed phase are larger than 1 micrometer. Over time, gravity will cause these particles to settle out of the mixture
aerosol
a heterogeneous mixture consisting of tiny particles or liquid drops dispersed in a gas
foam
a heterogeneous mixture in which a gaseous phase consisting of tiny bubbles is dispersed in a liquid or solid
emulsion
a heterogeneous mixture that contains two or more immiscible liquid phases
solution
a homogeneous mixture of 2 or more pure substances
intensity
a measure of the power contained in an acoustic wave; *the rate at which an acoustic wave transmits energy*
Lewis structure
a method of showing the covalent bonds and arrangement of a molecule using electron dot notation
diatomic
a molecule consisting of two atoms
polyatomic molecule
a molecule of three or more atoms
gamma decay
a nucleus sheds extra energy by emitting a gamma ray - there is no change in the atom except the amount of energy in the nucleus is reduced
photon
a packet of electromagnetic energy. An elementary non-material "particle" that transmits the electromagnetic force in the standard model of matter.
dispersed phase
a phase that is a minority in a heterogeneous mixture and that is dispersed or suspended throughout the continuous phase
colligative properties
a physical property of a solvent that depends on the concentration of the solute particles and is not the kind of solute. Common colligative properties are freezing-point depression, boiling-point elevation, and osmotic pressure
alpha particles
a positively charged particle that is given off by some radioactive materials including uranium, plutonium, and polonium - these particles are now known to be nuclei of helium atoms with 2 protons and 2 neutrons
unit cell
a repeated structural unit from which a crystal lattice is assembled. A unit cell is classified by the arrangement of atoms it contains
triple bond
a strong covalent bond formed when nonmetal atoms share three pairs of electrons
double bond
a strong covalent bond formed when nonmetal atoms share two pairs of electrons
electrolyte
a substance that dissociates or ionizes in water to produce an electrically conductive solution
radar
a technology that uses electromagnetic waves to determine distance, direction, speed, or shape of an object by radio-wave echolocation.
semipermeable membrane
a thin, sheetlike material that selectively allows solvent particles to diffuse and blocks the passage of solute particles
gel
a two phase heterogeneous mixture in which dispersed solid particles form an open network throughout a liquid continuous phase, giving some rigidity to the mixture. A gel has some of the properties of a solid but is mostly liquid
sol
a two phase heterogeneous mixture in which the dispersed solid phase does not form an open network in the liquid continuous phase as in a gel. Its particles may still have some attraction for each other, producing a viscous liquid
overtone or harmonic
a wave whose frequency is a whole-number multiple of the fundamental wave's frequency (2 possible names)
immiscibile
not able to dissolve in another liquid. Used of liquids. The liquid phases of an emulsion are immiscible.
isotopic notation
notation that shows the chemical symbol, atomic number (bottom left), and mass number (top left) for an isotope of an element
nuclear bombardment reactions
nuclear change that occurs when a nucleus is struck by a high-energy particle or another nucleus - nuclear fission - releases millions of times more energy and particles than with alpha or beta decay - almost always artificially induced in a special nuclear reactor or particle accelerator to control the amount and rate of particle release
atomic number
number of protons in an atom - this number determines the identity of the atom - can be found on the Periodic Table in the top left corner of each sqare
Acidic
pH 1 - 6; has more hydronium ions
Neutral
pH 7; has equal number of hydroxide ions
Basic (alkaline)
pH 8 - 14; has more hydroxide ions
proton
particle fixed in the nucleus of an atom - has a single positive charge - more than 1800 times the mass of an electron
neutron
particle located in the nucleus - has no charge - slightly more mass than a proton
electron
particle that is much smaller than protons and neutrons - has single negative charge - mobile - occupies a spherical region surrounding the nucleus - the arrangement and number of these determines an atom's ability to form bonds with other atoms - all of these have the same mass
luminous objects
produce visible light. produces all possible wavelengths of visible light to form a continuous spectrum.
gamma ray
produced by changes in atomic nuclei, 10pm - 1fm. A photon in the highest frequency of the electromagnetic spectrum.
precipitation reactions
products separate from the solution and settle out as a solidg
nucleons
protons or neutrons - particles in the nucleus
infrasonic
refers to sound waves below the range of human hearing; sound waves with extremely low frequencies
energy levels
represent the regions where an electron with a certain amount of energy is most likely to be found - these do not have well defined boundaries and can even overlap in the quantum model - electrons with the lowest energy occupy the first _________ closest to the nucleus - each _________ has a limit of the number of electrons it can hold
free electron theory
same as the electron sea theory
ear drum or tympanic membrane
separates the outer ear from the middle ear; converts acoustic energy to mechanical motion by vibrating in response to extremely tiny sound vibrations of air in the auditory canal
ear canal
serves as a resonating chamber in the ear
miscible
soluble in another liquid. Used of liquids
percentage by mass
solution concentration found by taking the ratio of the mass of the solute to the mass of the solution and expressing it as a percentage
John Dalton
strengthened the Law of Definite proportions through his own experimentation and suggested that 1- an atom cannot be created or destroyed in a chemical reaction 2*- an atom cannot be subdivided into smaller particles 3 - elements are made of only atoms 4 - the atoms of an element are all alike 5 - the atoms of one element are different than the atoms of another element (their masses) - developed the core-envelope model
catalyst
substances that speed up a reaction or enable it to take place without being consumed or changed - denoted over the yield sign
mass number
sum of the number of protons and neutrons (nucleons) in the nucleus of an atom
electron sea theory
the accepted model for metallic bonding. Metal cations are surrounded by their nonlocalized valence electrons. The "sea" of negative charge holds the cations in place.
illumination
the amount of light. reflecting a light
angle of reflection
the angle that a ray of light or the like, reflected from a surface, makes with a normal to the surface at the point of reflection.
angle of incidence
the angle that a straight line, ray of light, etc., meeting a surface, makes with a normal to the surface at the point of the meeting.
octane C8H18
the antiknock properties of different grades of gasoline are rated comparing a given blend of gasoline to that containing 100% of this
dissociation
the breaking apart of the ions in a solid ionic compound by the action of the solvent to form a solution
compression
the crest of a sound wave; a point of high particle density
osmosis
the diffusion of a solvent through a semi-permeable membrane from a region of higher concentration of the solute to one of the lower concentration
nuclear binding energy
the energy that hold protons and neutrons together in the nucleus
oval window
the entrance to the cochlea
Boron Family
the family which contains the element which is used in LCD's.
William Derham
the first person to accurately measure the speed of sound through air (1708-1709)
cochlea
the fluid-filled inner ear that contains thousands of sensory hair cells and nerve endings
sound
the form of energy detectable by our ears
Henry's law
the greater the pressure of a gas on a liquid, the greater the mass of the gas that can dissolve in the liquid at a given temperature
woodwind
the instrument group whose pitch is varied by opening and closing keys
diaphragm
the large dome-shaped muscle that controls breathing
ground state
the lowest and most stable energy state an atom can have - atoms may occupy up to seven energy levels in the largest atoms at ___________ - when an atom is excited, it may occupy more than seven energy levels
solubility
the maximum amount of solute that can be dissolved in a given amount of a particular solvent at a specified temperature
concentration
the measured amount of a solute in a given amount of solvent; it may be measured in units of percentage by mass, specific gravity, moles per liter, or other units
boiling-point elevation
the number of degrees the boiling point of a solvent is increased per mole of dissolved solute particles. It is a colligative property of the solvent.
freezing-point depression
the number of degrees the freezing point of a solvent is reduced per mole of dissolved solute particles. It is a colligative property of the solvent
threshold of pain
the point at which sound becomes painfully loud and can permanently damage hearing
osmotic pressure
the pressure that must be applied to the solution side of a semipermeable membrane to prevent the net diffusion of the pure solvent through the membrane into the solution
reverse osmosis
the process of removing solutes from a solvent by applying a pressure greater than the osmotic pressure of the solvent, forcing the solvent from the solution side to flow through a semipermeable membrane, thus purifying it.
Periodic Law of the elements
the properties of the elements vary with their atomic numbers in a periodic way.
nuclear radiation
the rays and particles emitted by unstable nuclei
radioactivity
the release or emission of nuclear radiation
loudness
the response of your ear to the intensity of a sound wave
Tyndall effect
the scattering of light off dispersed or suspended particles in a heterogeneous fluid mixture; the definitive test that differentiates between a colloidal dispersion and a true solution
formula unit
the smallest ratio of elements in an ionic compound that describes its composition; the molecular formula of a covalent compound
threshold of hearing (TOH)
the softest sound detectable by the average young person's ear
nuclear chemistry
the study of changes that occur in the nuclei of atoms
solute
the substance dissolved in the solvent in a solution; the minority component in a solution
solvent
the substance that does the dissolving in a solution; the majority component in a solution
zero sum rule
the sum of oxidation numbers of all atoms in a compound must equal to zero because compounds are not electrically charged
alpha decay
the type of nuclear decay used in common household smoke detectors - atoms nucleus loses 2 protons and 2 neutrons, reducing its atomic number by 2 and mass number by 4
electron configuration
the unique arrangement of energy levels and the positions that electrons can take within those energy levels for a given number of electrons in the atom. Represented in orbitals s, p, d, f
atomic mass
the weighted average of masses of all the natural isotopes of the element - the relative abundance of each of an element's natural isotopes is taken into account to determine this - found directly under the abbreviation for each element on the Periodic Table
beta decay
this type of nuclear decay does not change the number of nucleons so mass number stays the same - however, a neutron is changed into a proton so the atomic number increases by 1 - this changes the atom into an isotope of another element
insoluble
unable to to dissolve in a certain solvent
binary covalent compound - naming
use prefixes to indicate the number of atoms (inorganic) - i.e. CO = carbon monoxide - element with positive oxidation number listed first
Robert Boyle
who defined an element as any substance that could not be decomposed into simpler substances.
high electron affinity
will gain some valence electrons
low electron affinity (the positives)
will lose or have very small part in sharing the electrons
low electron affinity
will lose some valence electrons
medium electron affinity
will share valence electrons
high electron affinity (the negatives)
will take or share the electrons
throat and sinuses
work together to form a resonating chamber for the voice (2 answers)
Metalloids characteristics
zig-zag except Al, kind of conductive, semi-conductors and very important in computers
Edinburgh, Scotland, in 1831
James Clerk Maxwell born and place of birth
Octaves
John Newlands organized the elements according to the law of _________.
light-emitting diodes
LED is a semiconductor device that emits light when current passes through it in one direction but not the other.
law of reflection
Law stating that the angle of an incident ray equals the angle of the reflected ray. Both angles are measured in relation to the normal at the point of incidence.
incandescence
Light produced by materials that are heated until they glow.
Trough
Lowest point of a wave.
Solubility
Maximum amount of a substance that will dissolve in a certain amount of solvent at a given temperature
pH scale
Measuring acidity easier
Lose
Metals _______ electrons! Da na na na nuh na na nuh
What are the 3 groups of elements?
Metals, Non-metals and Metalloids
Rest position
Midway between crest and trough.
What are atoms that do not bond called?
Monotomic
Metals
Most of these are ductile, or can be drawn into wire.
Metals
Most of these are good conductors of electricity and heat.
Refraction
Occurs when a wave moves from one medium to the other.
Interference
Occurs when two or more waves meet at the same point.
Monoprotic acid
One hydrogen to loose
Example of Triprotic acid
Phosphoric acid h3po4
Nodes
Points in a standing wave that experience no vertical displacement.
What are atoms that act naturally as more than 2 atoms?
Polyatomic
Arrhenius definition of base
Produces hydroxide ions in a water solution OH-
Rutherford's experiment
Proved that most of the atom must be empty space since most alpha particles went right through the gold foil, an atom's positive charges are concentrated in the nucleus where the alpha particles were deflected bouncing off the foil at sharp angles, and protons have the opposite charge of electrons
total internal reflection
Reflection of a light ray approaching the boundary between tow media from within the optically denser medium. --- occurs when the incident angle exceeds the critical angle for the two media.
specular reflection
Reflection of photons off a microscopically smooth surface in the same direction. An image of the light source can be formed from -
Base's limitation
Requires water in a liquid
Tyndall Effect
Scattering of a light beam as it passes through a colloid
Chemical symbols
Scientists represent elements by their ________ _________.
Most of water's special properties are due to
Shape and structure and shape of its polarity
Electromagnetic wave
The vibration does not require a substance.
Mechanical wave
The vibration goes through a substance.
cold light
Visible light produced by chemical reactions at temperatures far below those required for incandescence.
He
What is the periodic symbol for Helium.
H
What is the periodic symbol for Hydrogen.
I
What is the periodic symbol for Iodine.
Fe
What is the periodic symbol for Iron.
Mg
What is the periodic symbol for Magnesium.
Hg
What is the periodic symbol for Mercury.
Ne
What is the periodic symbol for Neon.
Ni
What is the periodic symbol for Nickel.
N
What is the periodic symbol for Nitrogen.
O
What is the periodic symbol for Oxygen.
P
What is the periodic symbol for Phosphorus.
Pt
What is the periodic symbol for Platinum.
Pu
What is the periodic symbol for Plutonium.
K
What is the periodic symbol for Potassium.
Ra
What is the periodic symbol for Radium.
Rn
What is the periodic symbol for Radon
Sl
What is the periodic symbol for Silicon.
Si
What is the periodic symbol for Silver.
Na
What is the periodic symbol for Sodium.
S
What is the periodic symbol for Sulfur.
Sn
What is the periodic symbol for Tin.
w
What is the periodic symbol for Tungsten.
U
What is the periodic symbol for Uranium.
As
What is the periodic symbol for arsenic.
Pb
What is the periodic symbol for lead.
metals
What type has low electron affinities?
metalloids
What type has medium electron affinities?
Monatomic
What type of elements occur as a single atom.
Diatomic
What type of elements occur as molecules of two atoms.
nonmetals
What types has high electron affinities?
Fire, Earth, Water, and Air
What were the names of Aristotle's four elements.
monochromatic
describes light that has the same wavelength so it is one color. lasers or LED produce single colors or wavelengths of light.
arrangement and number of electrons
determines how the atom will bond
electronegativity
determines strength and type of bond
chemiluminescence
(in chemical reactions) the emission of light by an atom or molecule that is in an excited state.
mole
(mol) the base SI unit for Avogadro's number of atomic or molecular particles; the mass of a substance containing Avogadro's number of particles; 1 mol=6.022 x 10 to the 23 power of particles
P shape contains ________ orbital(s) and ______ electrons
3, 6
precipitate
An insoluble solid produced by a chemical reaction that settles to the bottom of the liquid medium or formed when the concentration of a solid solute exceeds its solubility limit - denoted by a downward arrow
polyatomic ion
An ion made of two or more covalently bonded atoms that acts as a single charged particle.
virtual image
An optical illusion perceived by the visual system when processing diverging light rays reflecting off a mirror or passing through a lens. A -is upright and cannot be projected on a screen.
Continuous Phase
An unbroken phase that makes up most of a heterogeneous mixture in which other phases throughout the continuous phase
Brønsted-Lowry definition of an base
Any compound that accepts proton
Brønsted-Lowry definition of an acid
Any compound that is a proton donor
radio navigation
Any method of navigation using radio signals.
primary hue
Any single color of a small set of distinct colors that can be mixed to produce the other colors in a color system.
Arrhenius definition of an acid
Any substance that produces by hydrogen ions in a water solution H+
Oscillations
Are large, slower repetitive motions.
Vibration
Are small rapid repetitive motions.
Alkali metals
Because of the one valence electron this group is highly reactive.
Bases taste
Bitter
Dynamic equilibrium
Constant but continuously changing process equal amount going forward and backward
luster
Has a shine
Amplitude
Height from the rest position to crest. Half of the total wave length.
1912 discovered the atomic # and we use the table today
Henry Mosely
Foam
Heterogeneous mixture in which a gaseous phase consisting of tiny bubbles is dispersed in a liquid or solid
by bonding to form molecules and compounds
How can an atom fill an octet?
by EN numbers
How is electronegativity measured?
117
How many elements are there?
11
How many of the 92 naturally occurring elements are gasses at room temperature.
2
How many of the 92 naturally occurring elements are liquid at room temperature.
79
How many of the 92 naturally occurring elements are solid at room temperature.
The key acid In Your stomach is
Hydrochloric
Any substance that has ________________ first in its formula is an acid.
Hydrogen
Frequency
IS the rate at which cycles repeat. The symbol for it is f, and its unit is cycle per second or hertz (Hz)
Constructive interference
If a wave crest-to-crest (or trough-to-trough) meet, the wave increases in size at the point where they meet.
Column
In general. Neutral elements in the same ________of the periodic table have the same number of valence electrons.
Acid's limitation
In liquid or in water
coherent light
In-phase, monochromatic light waves from a single source.
Salt
Ionic compounds produced from an acid-base reaction positive base cation
pH meter
Is more accurate and electronic
oxidation number (ON)
The number of electrons that a bonded atom or ion must gain or lose (to return to its neutral state. Used for writing the formulas of mainly inorganic compounds.
Nobel Gasses
The only NATURALLY occurring monatomic elements.
principal focus
The point at which light rays initially parallel to the principal axis converge when focused by a concave mirror or converging lens; the focal point of incident parallel light rays.
focal point
The point at which nonparallel incident light rays are focused by a concave mirror or converging lens. The----- depending on the degree of divergence of the incident light rays. For parallel incident light rays, --- principal focus are the same point.
Diprotic acid
Two ionizable hydrogen atoms
Polyprotic acid
Two or more hydrogen's to use
Elements
What are substances that cannot be broken down into any other substances
Noble Gases; have all 8 valence electrons
What family has no EN? WHy?
atoms
What is everything made of?
Periodic Table of Elements
What is one of the most useful tools of science.
Al
What is the periodic Symbol for Aluminum.
Ar
What is the periodic symbol for Argon.
Ba
What is the periodic symbol for Barium.
Br
What is the periodic symbol for Bromine.
Ca
What is the periodic symbol for Calcium.
C
What is the periodic symbol for Carbon.
Cl
What is the periodic symbol for Chlorine.
Cr
What is the periodic symbol for Chromium.
Cu
What is the periodic symbol for Copper.
F
What is the periodic symbol for Fluorine.
Au
What is the periodic symbol for Gold.
valence electron
chemical bonds use?
gas in reaction
denoted by an upward arrow or (g)
aq
denotes in solution
endothermic
describes a reaction that absorbs energy from the surroundings - this energy is considered a reactant and is noted by a symbol over the yield sign or listed with the reactants - the delta sign or the letter Q denotes thermal energy (heat) - elec denotes electricity
supersaturated
describes a solution in which the solute concentration exceeds its normal solubility limit under existing conditions, a highly unstable condition that can result in rapid precipitation of the solute
unsaturated
describes a solution in which the solute concentration is below its solubility limit (additional solute can dissolve under the existing conditions)
saturated
describes a solution in which the solute's concentration is at its solubility limit (no additional solute can dissolve under the existing conditions)
chemical symbols
letters used to represent an element
incandescent
light bulbs produce about 0.8cd of light per watt of electrical power they use.
compounds with polyatomic ions - naming
list name of cation (positive oxidation number) - second list anion - use polyatomic ions full name with no prefixes necessary for ions - if anion is a singe element, use ide ending - use stock system for metals
positive oxidation number
lose electrons - includes metals
Metals
many pure _______are so soft that they can be cut with a knife.
cancer, 48
maxwell died of ---
binary ionic compound - naming
metal is named first and then the nonmetal with an "ide" ending - Stock system is used with metals having more than one oxidation number
Repetitive Motion
Is motion that occurs again and again.
Damping
Is the effect of friction on periodic motion.
Resonance
Is the opposite of damping.
Diffraction
Is the process of a wave bending around a corner or an object.
Period
Is the time takes to complete one cycle. Marked as T and its base SI unit is seconds.
Doppler Effect
A moving object pushes the air ahead of it closer together, causing the frequency of sounds in that air to increase.
Pulse
A single wave cycle of a vary short burst of waves.
microwave
EM waves with a relatively long wavelength - between radio waves and infrared. (support line-of-sight communications, high-speed data links, and high-accuracy radar.
Cycle
Each repeated motion.
Foucault Pendulum
Gives direct evidence that the earth turns on its axis.
Destructive interference
If two waves crest-to-trough meet, the waves disappear of are reduced at that point.
Pendulum
Is a mass attached to a rigid arm or flexible string.
Wave
Is a rhythmic disturbance moving from one place to another.
Beats
Is a wave occurs when slightly out-of-phase waves meet.
Pendulum
Is an osculation system which swings back and forth repeatedly.
Standing wave
Is composed of two waves of the same wavelength moving through each other in opposite direction.
Periodic motion
Motion that repeats at a constant rate. It is a type of repetitive motion.
Reflection
Occurs when waves bounce off a surface.
Cycle
One complete crest and trough.
visible light
The band of electromagnetic frequiencies human eyes can detect, extending from approximately 384 THz at the red end of the spectrum to 789 THz at the violet end.
electromagnetic spectrum
The entire frequency continuum of electromagnetic waves
Crest
The highest point of a wave.
speed of light (c)
The speed of any electromagnetic wave in a vacuum, approximately 3.00 X 10 to the 8th power m/s
radiotherapy
The use of high-energy radiation to treat cancers
terahertz band
a subset of the IR band extending from 300 GHz to 3 THz. It is used in medical imaging, low-energy astronomy, and other emerging technologies.
sonar
a system using transmitted and reflected underwater sound waves to detect and locate submerged objects or measure the distance to the floor of a body of water
auricle
also known as the outer ear; helps us determine the direction of a sound's source by blocking sounds coming from behind
resonance
amplifies sound; in your sinuses, this amplifies the sound of your voice
radio waves
electromagnetic waves in the frequency range extending from far below 300 Hz to 300 GHz, produced by the acceleration of electrons. (TV signals, radio signals, and radio astronomy.)
synthesizers
can produce nearly the full range of tones of most instruments as well as realistic imitations of other sounds
Robert Boyle
conducted an experiment on sound in 1660 by hanging a watch with an alarm in a vacuum; when no sound was heard, he *proved that a medium is required for sound to travel*
auditory nerve
conducts electronic signals from the sensory cells to the brain, which interprets the signals as sound
frequency
cycles per second of sound waves; measured in Hertz (Hz)
pitch
how high or low an audible tone sounds to the human ear
hydrophones
instruments used in early sonar that only received sounds produced by other objects rather than sounds produced by itself
vocal cords
the two flat pieces of tissue contained within the larynx that vibrate and produce many of the sounds of the human voice
ultraviolet (UV)
produced by the emission of photons during large changes of electron energy levels within atoms.
ultrasonic
refers to sound waves above the range of human hearing; sound waves with extremely high frequencies (typically above 20,000 Hz)
transducers
sonar instruments that produce and listen for short pulses of sound; produce "pings" like those often heard in submarine movies
solids, liquids, gases
sound travels fastest in ______, slower in _______, and slowest in most _____
331.4 m/s
the accepted speed of sound through air
tongue, teeth, lips
the chief anatomical parts that contribute to the formation of individual sounds (3 answers)
mechanical (amplification)
the type of amplification that focuses sound energy in one specific direction, such as a megaphone
electronic (amplification)
the type of amplification that uses electronic technology to make sound louder
natural frequency
the frequency at which an oscillating object experiences resonance
brass
the instrument group whose sound is produced by a vibrating air column; the longer the instrument, the lower the sound
percussion
the instrument group whose sound is produced when the instrument is struck; size and tension change pitch
sound navigation and ranging
the long form/meaning of the word "sonar"
decibel (dB)
the unit of measurement of sound intensity
fundamental
the lowest-frequency sound wave in a complex mixture of related harmonic tones
quality
the particular sound of an instrument; what makes any sound distinctive
amplification
the process of making a sound louder
acoustics
the study of controlling the sounds that reach our ears
hammer, anvil, stirrup (malleus, incus, stapes)
the three bones of the inner ear
source (vibrating), medium (like air), receiver (like an ear)
the three things required to produce sound
rarefaction
the trough of a sound wave; a point of lowest particle density
echolocation
using sound to "see" and determine the distance to and the direction of an object; used by bats and dolphins
