Chap. 4-6.6 – Flashcards
137 test answers
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| Properties of a beta particle? |
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charge is 1- mass #= 0
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| Beta Particle symbol? |
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βor e |
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| What is a Positron? |
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| positive electron |
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| Symbol for Positron |
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| β+ |
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| Properties of Positron |
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1+ charge mass #= 0
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| what are gamma rays? |
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| High energy radiation released when an unstable nucleus undergoes a rearrangement of its particles to give a more stable lower energy nucleus. |
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| Gamma Rays symbol |
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| y |
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| Properties of Gamma rays |
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0 mass 0 charge |
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| Proper Shielding for Alpha Particles? |
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| Paper and clothing |
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| Proper Shielding for Beta Particle? |
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| gloves and lab coat |
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| Proper shielding for gamma rays? |
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| lead shield or thick concrete wall |
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Balance this equation: 251 247 Cf -----> Cm 98 96 |
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251 247 4 Cf -----> Cm + He 98 96 2 |
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| Alpha's isotope |
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4 ;; ; ;He 2 |
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| Betas Isotope |
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0 ;; ;e -1; |
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| Gamma Ray isotope |
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0 ;; ;y 0; |
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| Positron Isotope |
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;0 ;; ; ;e +1 |
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| Alpha particle mass |
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| 4 amu |
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| Beta Particle Mass; |
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| 1/2000 amu |
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| Gamma ray mass |
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| 0 amu |
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| Define transmutation? |
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A nucleus is converted to a radioactive nucleus by bombarding it with a small particle. |
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| what is curie? |
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| measures the number of atoms that decay in one second. |
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| curie symbol |
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| ci |
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| Define rad |
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| measures the radiation absorbed by the tissues of the body. |
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| what does rad stand for? |
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| Radiation absorbed dose |
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| What is rem? |
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measures the biological damage.
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| what does rem stand for? |
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| radiation equivalent |
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| 1Ci =___Bq |
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| 3.7x10^10 |
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| 1Gy=___ rad |
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| 100 rad |
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| 1Sv=____ rem |
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| 100 rem |
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| what is becquerel? |
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| one disintegration per second |
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| becquerel symbol |
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| Bq |
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| What is gray? |
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| = 100 rads |
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| gray symbol |
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| Gy |
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| what is sievert? |
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| = 100 rems |
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| sievert symbol |
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| Sv |
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| Define radiation isotope |
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| an isotope that emits radiation |
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| Define decay curve |
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| a diagram of the decay of a radioactive isotope. |
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| KNOW DECAY CURVE DIAGRAM ON PG 154 |
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| What does PET stand for? |
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| Positron emission tomography |
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| Define PET |
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| positron emitters with short half lives are used in an imaging method called PET |
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| Define Chain reaction |
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| occurs when a critical mass of uranium undergoes fission so rapidly that the release of a large amount of heat and energy results in an atomic explosion. |
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| Define Fission |
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a large nucleus is bombarded with a small particle. The nucleus splits into smaller nuclei. Several neutrons and a great amount of energy are released. |
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| Define fusion |
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Occurs at extremely high temperatures(100 000 000°C). Combines small nuclei into larger nuclei. Releases large amounts of energy. Occurs continuously in the sun and stars. |
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| Define Scan/Scanner |
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| used to produce an image of the organ, moves slowly across patients body above region where the organ containing the radioisotope is located |
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| Name some common uses of radioactivity in medicine |
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p-32 Treatment of leukemia I-125 Treatment of brain cancer |
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| Define Carbon Dating |
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| use half life of carbon-14 (5730 years) to calculate the length of time since the plant died. |
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| how many years is carbon-14 ? |
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| 5730 years |
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| KNOW EQUATIONS FOR HALF LIVES- STUDY PAPER |
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| Why is fusion a better energy source than fission? |
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| because fusion reactions occur continuously in the sun and other stars, providing us with heat and light. |
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| TO FIND g FOR HALF LIVES GO TO PG 154 |
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| How do you figure out the number of valence e- in group A? |
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| the # of valence e- is the number of e- in the s and p subshells of the outer shell. |
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| How do you know how many dots for e- dot structure? |
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ex: H20 H= group # 1 O= group # 6 1x2 +6= 8 dots |
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| Define octet rule |
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Is 8 valence electrons. Is associated with the stability of the noble gases. The process of acquiring an octet involves the loss, gain, or sharing of valence electrons.
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| Define Cation |
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positive charges |
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| Define Anion |
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| negative charge |
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| When an atom has and overall charge it is called an? |
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| ion |
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| Define ionization energy |
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| energy it takes to remove a valence e- |
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| Metals have ___ionization energies and nonmetals have___ ionization energies. |
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metals= lower nonmetals= higher |
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| Because ionization energies of metals if group 1A, 2A, & 3A are low, these metal atoms readily lose thier valence e- to____? In doing so they acquire the e- configuration of a noble gas ( 8 valence e-) and form ions with ____ charges. |
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nonmetals
positive |
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| charge of group 1A? |
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| 1+ |
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| Charge of group 2A? |
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| 2+ |
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| charge of group 3A? |
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| 3+ |
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| charge of group 5A? |
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| 3- |
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| Charge of group 6A? |
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| 2- |
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| Charge of group 7A? |
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| 1- |
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balance: Mg 2+ N 3- |
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| Mg3N2 |
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| Name ionic compound NaF |
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| Sodium Fluoride |
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| Name ionic compound Al2O3 |
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| Aluminum oxide |
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| Ionic compounds end in ___? |
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-ide metal than nonmetal ending in -ide |
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| The name of covalent compounds need ____? |
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| prefixes |
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| Prefix for one |
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| mono |
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| prefix for two |
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| di |
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| prefix for 3 |
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| tri |
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| prefix for 4 |
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| tetra |
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| prefix for 5 |
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| penta |
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| prefix for 6 |
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| hexa |
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| prefix for 7 |
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| hepta |
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| prefix for 8 |
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| octa |
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| prefix for 9 |
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| nona |
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| prefix for 10 |
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| deca |
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| ionic compound has? |
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| metal and nonmetal |
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| covalent compounds have? |
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| 2 nonmetals |
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| Define polar covalent |
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| when e- are shared unequally |
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| If the atoms have electronegativity differences of 0.4 or less that it is a ___? |
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| nonpolar covalent bond |
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| electronegativity difference of 0.5-1.6 than it is a ___? |
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| Polar covalent bond |
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| Electronegativity differences of 1.7 or more than it is a ___? |
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| ionic bond |
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| Define ionic bond |
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Ionic compounds consist of positive and negative ions. An ionic bond is an attraction between the positive and negative charges. In an ionic formula, the total charge of the positive ions is equal to the total charge of the negative ions. They balance out to zerototal positive charge = total negative charge |
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| define tetrahedral |
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Four electron groups. Repulsion is minimized by placing four electron groups at angles of 109° [image] |
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Define covalent bond
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| atoms share electrons to complete octets |
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| Define trigonal pyramidal |
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Three electron groups bond atoms and the fourth one is a lone (nonbonding) pair. Repulsion is minimized with 4 electron groups [image] |
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| Define trigonal planar |
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arrangement of three e- groups as far apart as possible. Repulsion is minimized with 3 electron groups at angles of 120° [image] |
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| Define Valence- shell electron pair repulsion theory (VSEPR) |
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| indicates that the e- groups will move as far apart as possible to reduce the repulsion between their negative charge. |
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| define dipole |
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| a polar covalent bond that has a separation of charges |
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| Define nonpolar covalent bond |
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| a covalent bond between atoms with identical or very similar electronegativity values. |
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| Define resonance structures |
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| when two or more electron dot formulas can be written and shown with a double headed arrow |
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| Define Linear shaped |
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are two electron groups bonded to the central atom.
To minimize repulsion, the arrangement of two electron groups is 180° or opposite each other. [image]
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| define Bent |
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Two electron groups are bonded to atoms and two are lone pairs (4 electron groups). Four electron groups minimize repulsion(~109°). [image] |
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| Define nonpolar molecule |
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Contains nonpolar bonds. Cl–Cl H–H
Or has a symmetrical arrangement of polar bonds. O=C=O |
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| Define polar molecule |
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Contains polar bonds. Has a separation of positive and negative charge called a dipole indicated with d+ and d-. Has dipoles that do not cancel. d+ d- • • H–Cl H—N—H N dipole |
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| Define chemical change |
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Reacting substances form new substances with different compositions and properties. A chemical reaction takes place. |
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| define chemical reaction |
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A chemical change produces one or more new substances. There is a change in the composition of one or more substances. |
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| Define coefficient |
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| whole numbers in front of formulas |
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| define combination reaction |
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| two or more elements or compounds bond to form one product |
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| S(s) + 02(g)-----> _____ |
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S(s) + 02(g)-----> SO2(g)
(Combination) |
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| Define Decomposition Reaction |
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| reactant splits into two or more simpler products |
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| 2HgO(s)----> _____ |
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2HgO(s)---->2Hg(l)+ O2(g)
(decomposition) |
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| Define single replacement Reactions |
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| reacting element switches place with an element in the other reacting compound |
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| Zn(s)+2HCl(aq)--> ___ |
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Zn(s)+2HCl(aq)--> ZnCl2(aq)+ H2(g)
(single replacement) |
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| Define double replacement |
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| the positive ions in the reacting compounds switch places |
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| BaCl2(aq) + Na2SO4(aq) ----> _____ |
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BaCl2(aq) + Na2SO4(aq) ----> BaSO4(s) + 2NaCl(aq)
(double replacement) |
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| Define oxidation |
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| loss of electrons |
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| Define Reduction |
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| the gain of electrons |
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| define oxidation-reduction reaction (redox) |
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| e- are transferred from one substance to another |
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| Reactants are written on the _____side |
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| left |
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| Products are written on the ____side |
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| right |
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| define physical change |
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The identity and composition of the substance do not change. The state can change, or the material can be torn into smaller pieces. |
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| what is Avogadros number? |
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| 6.02x10^23 |
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| 1 mole= ____ |
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| 6.02x10^23 |
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particles __________________ 1mole |
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6.02x10^23 particles _______________ 1 mole |
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| convert 4.00 moles of Fe to atoms of Fe. |
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4.00moles Fe atoms x 6.02x10^23 Fe atoms ___________________ 1 mole fe atoms
= 2.41x10^24 Fe atoms |
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| Convert 3.01x10^24 molecules of CO2 to moles of CO2 |
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3.01x10^24 CO2 Molecules X 1 mole CO2 Molecules _________________________ 6.02x10^23 CO2 molecules = 5.00 moles of CO2 molecules |
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Given:1.75 moles of CO2 Need: molecules of CO2 |
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1.75moles CO2 x 6.02x10^23 molecules CO2 _______________________ 1 mole CO2 = 1.05x10^24 molecules od CO2 |
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| How many carbon atoms are present in 1.50 moles of aspirin C9H804? |
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1.50 moles of C9H804 X 9 moles C X 6.02x10^23 C atoms __________ _______________ 1 mole C9H804 1 mole of C atoms = 8.13x10^24 C atoms |
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| Define Molar Mass |
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the mass of one mole of a substance the atomic mass of an element expressed in grams
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| Molar masses of S and O |
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1 mole x 32.1 g S _________ =32.1g of S 1 mole S
3 moles O x 16.0 g O _______________ =48.0 G of O 1 mole O
32.1g of S 48.0g of O ____________ MM= 80.1g of SO3 |
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Calculate grams of silver using Molar mass Given: 0.750 mole of Ag |
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0.750mole Ag x 107.9g Ag _______________ = 80.9 g of Ag 1 mole Ag |
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| In the reaction of Fe and S how many moles of S are needed to react with 6.0 moles of Fe? |
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2Fe(s) + 3S(s) --------> Fe2S3(s)
6 moles Fe X 3 moles S ____________ = 9.0 moles of S 2 moles Fe |
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| Define Mole to Mole factors |
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| between reactants and between reactants and products |
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| In the formation of smog, nitrogen reacts with oxygen to produce nitrogen oxide. Calculate the grams of NO produced when 1.50 moles of 02 reacts |
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N2(g) + O2(g) ------> 2NO(g)
1.50 moles 02 X 2 moles NO X 30.0g NO __________ __________ = 90.0g of NO 1 mole O2 1 mole NO |
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| how many dots does Hydrogen need? |
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| 2 |
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| how many dots does Be need? |
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| 4 |
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| how many dots does B need? |
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| 6 |
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| Which elements can expand their octet to 10,12, or 14 dots? |
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| Sulfur, Phosphorus,chlorine, bromine, and iodine |
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