BJU Physical Science Chapter 12-21 (CCA Final Exam Review)

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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


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