Physics U3 & HW
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| Anything that occupies space and has inertia(mass) | Matter
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| Smallest subdivision of substance having the physical properties of the substance | Molecule
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| what determines the state a molecule is in and what are the types of states? | the degree of attraction; solid, liquid, or gas
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| Has the strongest molecule attraction | Solid
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| Has the weakest molecule attraction | Liquid
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| which type of molecule attraction repels | the gas
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| Smallest particle of an element that has the characteristic properties of that element and can combine chemically with one or more atoms of another element | Atoms
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| What are the 4 atoms of the Greek | earth, fire, water and air
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| Who compared the atoms to hooks and eyes in 1808? | Dalton
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| Who compared the atom to plum pudding | Thompson
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| Who compared the atom to the solar system in 1913 | Bohr
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| Any material that has definite constant composition | Substance
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| Elements, cannot be decomposed to simpler substances by ordinary means | Simple substance
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| These are compounds | Complex substance
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| A chemical union of two or more elements in definite proportions | Complex substance
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| Give an example of a substance | Salt also a complex substance
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| Give an example of simole substance | sodium and oxygen
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| This is the positive charged center of an atom that contains most of the atom's mass | Nucleus
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| The nucleus of an atom contains what percent of the mass? | 99%
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| What was Bohr's Theory | The atom is represented as a miniature solar system analogous to the sun with the planets revolving around it
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| Negatively charged particles that circle the nucleus each in its own path or shell | Orbital electrons
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| How are electrons grouped | by their shells or energy levels
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| What is the binding energy of a shell that is close to the nucleus | The binding energy is strong but the energy shell is weak
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| What is the binding energy of a shell that is farther away from the nucleus | The binding energy is weak but the energy shell is strong
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| The periodic table is an arrangement of | all the electrons in an orderly series
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| Who developed the periodic table and how did he arrange the electrons | Medndleev; accroding to the lowest atomic number to the highest or how many electrons in the outer shell
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| How may groups are in the periodic table | 8 vertical
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| Represents families of elements that have similar chemical properties | Groups
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| What is the exception in the periodic table | Hydrogen
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| Group 1 is | Alkali metals and has 1 electronin the outer shell
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| group 2 | has 2 electrons in the outer shell
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| group 7 are | halagens
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| group 8 are | nobel gases(inhert elements)
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| The horizontal rows of the periodic table are based upon what and how many are there? | Based on the number of electron shells and there are 7
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| All of the elements in each row of the periodic table have the same number of what but different _________ properties. | Electron Shells; Chemical
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| ªᵣXⁿ Define each letter | a=mass #; r=Atomic #; X=Element; n=Valence #
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| the shell number is referred to as | The quantum number
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| The outer most shell does not what | have to contain the maximum number of electrons
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| No outer shell contains more than | 8 electrons
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| All atoms seek to have 8 electrons in its outer shel, what is this | octet rule
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| What is the formula to calculate the maximum number the electrons a shell can hold | 2n² (n=the energy shell)
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| how many electrons can the n shell hold | 2(4)²= 16x 2= 32
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| A nucleus contains | Protons and neutrons
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| Positive charge,equal and opposite to an electron | Protons
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| How much heavier is a proton than an electron | 1828 times heavier
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| Has a mass slightly greater than a proton | neutron
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| Why is a neutron slightly greater than a proton | because it is really a proton and an electron united
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| What are the building blocks of an atom | protons, neutrons, and electrons
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| Why must the number of protons be equal to the number of electrons | because an atom is always going to try to keep a neutral charge of 0
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| Is determined by the number of electrons in the outer shell of the atom | Valence #
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| What are the positive valence #'s | 1 outer shell electron +1; 2 outer electrons +2; 3 outer electrons +3
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| What are the negative valence #'s | 7 outer electrons -1; 6 outer electrons -2; 5 outer electrons -3
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| The number of (+) charges/protons in the nucleus of an atom | Atomic #
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| What is the symbol for the atomic # | z
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| the total number of protons and neutrons(nucleons) in the nuceus of a atom | Mass # or atomic #
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| Symbol for atomic # or mass # | A
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| Atoms that have the same number of nuclear protons(same atomic number) but different number of nucleur neutrons(different mass number) | Isotopes
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| What are the two types of chemical bonding | Covalent and Ionic
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| Sharing of the electrons to achieve the Octet Rule and has a weaker bond | Covalent bonding
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| Ionization must occur in an attenpt to achieve the octet rule and has a strong bond | Ionic bonding advanced
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| Give an example of a covalent bond | water two atoms of hydrogen(each with 1 electron in its outer shell) share their electrons with 1 atom of oxygen that has 6 electrons in its outer shell
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| Give an example of ionic bonding | NaCl Chlorine with 7 electrons in its outer shell steals the 1 electron in the sodiums outer shell which causes them to become oppositely charged. They are magnetically attracted to each other in bond
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| What are not involved in the ionization process | protons
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| The process of converting electrically neutral atoms to electrically charged atoms through the addition or removal of orbital electrons | Ionization
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| What charge does the ion have if the electron is removed | +
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| what charge does the ion have if the electron is added | -
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| Argon | Ar
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| Barium | Ba
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| Beryllium | Be
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| Calcuim | Ca
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| Cobalt | Co
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| Gold | Au
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| Helium | He
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| Hydrogen | H
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| Iodine | I
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| Iron | Fe
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| Lead | Pb
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| Oxygen | O
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| Radium | Ra
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| Radon | Rn
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| Silver | Ag
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| Soduim | Na
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| Sulfer | S
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| Tungsten | W
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| Uranium | U
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| Arsenic | As
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| Silicon | Si
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| Gallium | Ga
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| Six ways to bring about ionization | X-ray bombardment of matter/Electrons stream bombardment of matter/Spontaneous breakdown of radioactive nuclides/Light ray bombardment of certain elements/chemical ionization/Thermionic emission
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| Explain x-ray bombardment | Dislodging orbital electrons/ Photon interaction
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| Explain Electron stream bombardment | Dislodging orbital electons/ x-ray tibe
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| Explain spontaneous breakdown of radioactive nuclides | Decaying isotopes
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| Explain the light ray bombardment of certain elements | light causes electrons to be emitted from certain metals-cesium and potassium
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| Explain chemical ionization takes place | electrolysis/ NaCl with electrodes
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| Explain where thermoionic emission takes place | Filament of the x-ray tube
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| energy emitted and transferred through matter(irradiated) | radiation
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| removes electrons | ionizing radiation
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| What are the types of ionizing radiation | electromagnetic and particulate
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| Electromagnetic ionizing radiation has | no mass, no charge and a constant velocity of speed
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| Particulate ionizing radiation has | has mass, may or may not have a charge, velocity varies
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| x-rays and gamma rays are | x and Y electromagnetic ionizing radiation
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| Alpha and beta rays are | Particulate ionixing radiation (a) and (B)
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| What is the difference between the x-ray and the gamma ray | The point of origin
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| Where does x-rays come from | The shells of the atoms
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| Where does gamma radiation come from | The nucleus of an atom
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| High spped electrons | Beta particles
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| Generally negatively charged electrons(particulate radiation) | Beta negatrons
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| Postively charged electrons (particulate radiation) | Beta Positrons(they are small but penetrate deep)
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| Helium atom stripped of all its electrons | alpha particles (these are large but dont travel fast)
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| What make up alpha particles | 2 protons and 2 neutrons (double ionized helium atom)
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| Process which results in the transmutation of one element to another | radioactivity (Uranium-Radium-Lead)
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| In the decay of radioisotopes the nuclues emitts | alpha, gamma, and beta radiation which cause transformation
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| This is the most commonly occuring emission | Beta emission
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| During beta emission what happens | A beta electron is emitted with a neutrino, a neutron converts to a proton, and this increase the atomic number by one while the mass number stays the same
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| When the z number increases what happens | the atom becomes an ion and must pull an electron to stabilize itself/ this changes the atom from one element to another
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| Beta(-1 charge) | high speed electron that was attached to a neutron
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| Alpha(+2 Charge) | two protons and two neutrons
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| Neutron(0 Charge) | A neutron
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| This type of beta emission only involves what | the negatively charged particles(beta negatrons)
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| Alpha emission is a | Violent process and is a Helium nuclues
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| When Alpha is emitted the mass number ______ and the atomic number______ | is reduced by 4 / is reduced by 2
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| Some___ are pure beta emotters and some are pure Alpha emitters but most all emit Gamma | isotopes
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| Atoms that have the same atomic number but different atomic mass numbers/ Atoms that have the same number of protons but different nuetrons | Isotopes
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| Atoms with the same number of nucleons(mass Number) but different numbers of nuetrons and protons/ Atoms with the same Mass number but different atomic number | isobars
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| Atoms with the same number of neutrons but different number of protons/ Different atomic numbers and different atomic mass numbers but constant value for A-Z | isotones
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| Same atomic number and same atomic mass number | isomers
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| isomers exist in different energy states because | of differences in the nucleon arrangement
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| The ability of some nuclides to undergo spontaneous breakdown emitting ionizing radiation | Radioactivity
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| When does radioactivity occur | naturally and artifically
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| What are the naturally radioactive elements | thorium/ uranium/ actinium
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| The period of time required for a quantity of radioactivity to decay to one half of its initial value | Half-Life
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| What is the formula for Half-Life | (T1/2)
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| Which of the following statements is true regarding our unterstanding of atomic structure | Rutherford described the nucleus
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| In the rendering of the atom J.J. Thompson | Uniform positive electrification was theorized
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| The periodic table represents the element in the order of | atomic number
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| Approximately how many known elements are there | 100
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| The only element that is not in any group of the periodic table is | hydrogen
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| The horizontal rows in the periodic table are called | peroids
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| As you move from left to right across the periodic table what happens to the number of outer shell electrons from one element to the next | it increases by 1
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| Which group in the peroidic table contains elements that have only one electron in the outer shell | Alkali metals
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| Which of the following is a traditional element | Tungsten
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| Atoms with all three electrons in the outer shell | have 3 valence electrons
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| In the periodic table of the the elements the group number identifies the | number of electrons allowed in the outer shell
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| All of the following are elements except | Steel
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| How many atoms are there in one molecule of sodium bicarbonate | 6
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| Which of the following physists had a major part in decreasing the atom as we know it today | Bohr
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| which of the following statements is true | in 1 yr light can travel approximately 10^16m
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| The periodic chart of elements is attributed to | dimitri mendeleev
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| Rutherford made what significant contribution to science | description of the nuclear atom
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| Which of the following statements about atoms are true | Most of the atoms are made of empty space
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| Which of the following statements about atoms are true | Atoms that have the same atomic number are atoms with the same atomic element
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| If I129/53 is a stable, electrically neutral atom, how many neutrons are there | 76
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| When oxygen (16/8 O) combines with atom of hydrogen (1/1 H) to form water the resultant molecule has a total of | 10 protons
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| The atomic number of an atom is given by the number of | protons plus neutrons
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| The atomic number | is the number of protons
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| Isotopes are atoms | of the same element
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| Electrons in the M-shell | do not exceed 18 in number
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| 12/6 C and 14/6 C have the same | number of protons
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| The binding energy of an electron to a nucleus is | higher for an L-shell electron than an M-shell electron
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| How many nucleons does 131/53 I have | 131
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| The number of protons in the nucleus is called the | atomic number
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| A neutron has approximately | 1amu(mass) and no charge
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| How many different types of nucleons are there | 2
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| Tungsten 184/74 W has how many neutrons | 110
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| what is the maximum number of electrons permitted in the N-shell | 32
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| Regarding atomic nomenclature | atomic mass number is a whole number
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| the following atoms are all stable which has the highest k-shell electron binding energy | Hg(mercury)
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| Alpha particle | radiation that can not penetrate a sheet of paper
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| beta particle is | a particle with a charge of -1.602x10(-19)C
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| Cyclotron is | A particle used to Produce radioisotope
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| Gamma Rays are | uncharged radiation : highly penetrating
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| Gold is | A stable atom that can be made radioactive
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| Isotopes are | atoms with the same number of protons but different number of neutrons
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| Radioactive is | a substance composed of all atoms with unstable nuclei
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| Radioactivity | Spontaneous emission of energy or p[articles from unstable nuclei
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| Radioisotopes are | usually produced by particles from common elements
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| Uranium is | an atom that is naturally radioactive
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| Whena radioisotope emits beta particle | a neutron is converted into a proton
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| Isotopes are | atoms that have the same atomic number but different atomic mass numbers
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| Beta emission results in | the gain of a proton
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| Alpha emission results in | the loss of 4 amu
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| After beta emission the nucleus has | increased in Z number by 1
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| Radioisotopws have what type of nuclei | an unstable one
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| Electrons are arranged how | in orbits around the nucleus
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| What is true about radioisiotopes regarding decay | The percentage of atoms decaying per unit of time is constant
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| The difference between electrons and beta particles is | their origin
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| In the air gamma rays | do not normally travel farther than 10 m
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| What could be the most penetrating radiation | 100 keV
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| The difference between the x-ray and gamma rays is | their origin
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| X-rays have | no mass no charge
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| What type of radiation is emitted from the outside of the nucleus | x-rays
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| As compared with particulate radiation electromagnetic radiation | has a higher electrostatic charge
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| Electromagnetic radiation ionizing radiation comes from | inside and outside of the nuclei
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| x-rays and gamma rays are examples of electromagnetic radiation both have | no electricostatic charge
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| what is an example of ionizing radiation | energetic protons
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| what are the two principle classes of ionizing radiation | particulate and electromagnetic
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| what is not ionizing radiation | therapeutic ultrasound
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