![Bohr model](http://s1.studyres.com/store/data/001767518_1-4b458b5092dadc04284a17174e190cb7-300x300.png)
Bohr model
... move to the plate and the current rises accordingly. • For mercury atoms, when V=4.9V, the electrons make inelastic collision and leave the atom jump to a high orbit (n=2). The original electrons move off with little energy and could not reach the plate and thus reduce the current. • As V is increas ...
... move to the plate and the current rises accordingly. • For mercury atoms, when V=4.9V, the electrons make inelastic collision and leave the atom jump to a high orbit (n=2). The original electrons move off with little energy and could not reach the plate and thus reduce the current. • As V is increas ...
Gupta 2014 Credit: Google Images for the pictures Chapter 1
... Titration is a method to determine the molarity of unknown acid or base. In titration, an acid or base of unknown molarity is titrated against a standard solution (whose M is known) of acid or base.The end point in a titration is indicated by a color change by the indicator. Indicators are weak acid ...
... Titration is a method to determine the molarity of unknown acid or base. In titration, an acid or base of unknown molarity is titrated against a standard solution (whose M is known) of acid or base.The end point in a titration is indicated by a color change by the indicator. Indicators are weak acid ...
SOLUBILITY RULES FOR IONIC COMPOUNDS IN WATER
... 19. nitrogen monoxide, nitrogen dioxide, dinitrogen monoxide, dinitrogen tetroxide, dinitrogen pentoxide 20. hydroiodic acid, hypoiodous acid, iodous acid, iodic acid, periodic acid 21. (a) ...
... 19. nitrogen monoxide, nitrogen dioxide, dinitrogen monoxide, dinitrogen tetroxide, dinitrogen pentoxide 20. hydroiodic acid, hypoiodous acid, iodous acid, iodic acid, periodic acid 21. (a) ...
Are diglycolamide ligands hard or soft Lewis bases?
... Pearson’s concept of Hard/Soft Acids/Bases (HSAB) in coordination chemistry – recapitulation Chemical hardness/softness of ligand molecules (L) can be considered in terms of the amount of electron density donated by the ligand (Lewis base) to the central metal ion (Lewis acid) in the complex. Hard ...
... Pearson’s concept of Hard/Soft Acids/Bases (HSAB) in coordination chemistry – recapitulation Chemical hardness/softness of ligand molecules (L) can be considered in terms of the amount of electron density donated by the ligand (Lewis base) to the central metal ion (Lewis acid) in the complex. Hard ...
NAME PRACTICE: QUANTUM CONFIGURATIONS 1) Each of the
... 2) The kinetic energy of photons striking the metal’s surface must equal that of the emitted electron. 3) The kinetic energy of photons striking the metal’s surface must be less than that of the emitted electrons 4) The kinetic energy of photons striking the metal’s surface must be greater than or e ...
... 2) The kinetic energy of photons striking the metal’s surface must equal that of the emitted electron. 3) The kinetic energy of photons striking the metal’s surface must be less than that of the emitted electrons 4) The kinetic energy of photons striking the metal’s surface must be greater than or e ...
Hybridization and St..
... Hybridization also occurs in compounds of beryllium. The electron configuration if Be is 1s22s2. It would appear to have no half-filled orbitals with which to form covalent bonds. ...
... Hybridization also occurs in compounds of beryllium. The electron configuration if Be is 1s22s2. It would appear to have no half-filled orbitals with which to form covalent bonds. ...
Midterm Review Packet - Mrs. McKenzie`s Chemistry and ICP Classes
... 10. In an ionic bond, __________ atoms of ________________ charge are held together by _________________________ attraction. 11. The part of an atom that has a neutral charge is a _______________________. 12. Most of the mass of an atom is found in the _____________________. 13. A pure substance mad ...
... 10. In an ionic bond, __________ atoms of ________________ charge are held together by _________________________ attraction. 11. The part of an atom that has a neutral charge is a _______________________. 12. Most of the mass of an atom is found in the _____________________. 13. A pure substance mad ...
Types of Measurement
... Two main kinds of compounds 1. Ionic: made up of ions of opposite charge A. strong electrostatic force of attraction; ionic bond B. electrons are transferred 2. Covalent: made up of two or more nonmetals A. electrons are shared ...
... Two main kinds of compounds 1. Ionic: made up of ions of opposite charge A. strong electrostatic force of attraction; ionic bond B. electrons are transferred 2. Covalent: made up of two or more nonmetals A. electrons are shared ...
King Abdulaziz University, Department of Physics, Jeddah
... In the absence of an electrical field, electrons move with randomly distributed thermal velocities. ...
... In the absence of an electrical field, electrons move with randomly distributed thermal velocities. ...
Atomic Theory (2
... 1.) What is an ion? 2.) How are ions formed? 3.) Why do ions form readily? (Be specific- in terms of stability) 4.) What is an anion? 5.) What is a cation? 6.) What type of elements form anions? 7.) What type of elements form cations? 8.) What is the relationship between valence electrons and ionic ...
... 1.) What is an ion? 2.) How are ions formed? 3.) Why do ions form readily? (Be specific- in terms of stability) 4.) What is an anion? 5.) What is a cation? 6.) What type of elements form anions? 7.) What type of elements form cations? 8.) What is the relationship between valence electrons and ionic ...
Chapters 6, 8
... 1. Find charges of both ions (from position in periodic table); write cation and anion with charges. 2. The sum of charges must be zero. Find out how many of each ion you must have. 3. Put index next to each ion indicating how many ions of that kind there is in the compound. Erase charges of both io ...
... 1. Find charges of both ions (from position in periodic table); write cation and anion with charges. 2. The sum of charges must be zero. Find out how many of each ion you must have. 3. Put index next to each ion indicating how many ions of that kind there is in the compound. Erase charges of both io ...
Many-Electron Atoms Thornton and Rex, Ch. 8
... In principle, can now solve Sch. Eqn for any atom. In practice, -> Complicated! ...
... In principle, can now solve Sch. Eqn for any atom. In practice, -> Complicated! ...
Chemistry I - Net Start Class
... 114. Calculate the mass of 8.50 x 1023 oxygen molecules. 115. A crude sample of Ag2O has a mass of 50.0 g. It contains 25.0 g of Ag2O. What is the percent of silver in the crude sample? 116. If 1.54 grams of an oxide of osmium (Os) are analyzed and found to contain 1.15 grams of osmium, what is the ...
... 114. Calculate the mass of 8.50 x 1023 oxygen molecules. 115. A crude sample of Ag2O has a mass of 50.0 g. It contains 25.0 g of Ag2O. What is the percent of silver in the crude sample? 116. If 1.54 grams of an oxide of osmium (Os) are analyzed and found to contain 1.15 grams of osmium, what is the ...
Chemistry Post-Enrolment Worksheet C
... of an oxygen atom and a hydrogen atom and has an overall 1- charge. Brackets can be used if we need more than one of a polyatomic ion in our formula. e.g. ammonium carbonate is made up of ammonium ions, NH4+ , and carbonate ions, CO32In order for the charges to balance we need two ammonium ions for ...
... of an oxygen atom and a hydrogen atom and has an overall 1- charge. Brackets can be used if we need more than one of a polyatomic ion in our formula. e.g. ammonium carbonate is made up of ammonium ions, NH4+ , and carbonate ions, CO32In order for the charges to balance we need two ammonium ions for ...
Chemistry Standards Checklist
... SCSh5. Students will demonstrate the computation and estimation skills necessary for analyzing data and developing reasonable scientific explanations. a. Trace the source on any large disparity between estimated and calculated answers to problems. b. Consider possible effects of measurement er ...
... SCSh5. Students will demonstrate the computation and estimation skills necessary for analyzing data and developing reasonable scientific explanations. a. Trace the source on any large disparity between estimated and calculated answers to problems. b. Consider possible effects of measurement er ...
Chemistry Nomenclature Notes
... -They become negatively charged and are called anions. -The size of the negative charge is determined by the number of electrons gained. -The number of electrons gained is determined by the proximity of Noble gas. -Named by dropping the ending and adding an ‘ide’ ending Ex: Chlorine is a group 7 ele ...
... -They become negatively charged and are called anions. -The size of the negative charge is determined by the number of electrons gained. -The number of electrons gained is determined by the proximity of Noble gas. -Named by dropping the ending and adding an ‘ide’ ending Ex: Chlorine is a group 7 ele ...
Multi-electron atoms have interactions between electrons, not just
... Higher values for "l" translate to higher energies for the electron! For convenience, and partially for historical reasons, we use letters to designate the different subshells. The rest follow the ...
... Higher values for "l" translate to higher energies for the electron! For convenience, and partially for historical reasons, we use letters to designate the different subshells. The rest follow the ...
200 ways to pass the regents
... 83. The elements in Group 1 are the alkali metals. 84. The elements in Group 2 are the alkaline earth metals. 85. The elements in Group 17 are the halogens. 86. The elements in Group 18 are the noble gases. 87. Use Table S to compare and look up the properties of specific elements. 88. Energy is rel ...
... 83. The elements in Group 1 are the alkali metals. 84. The elements in Group 2 are the alkaline earth metals. 85. The elements in Group 17 are the halogens. 86. The elements in Group 18 are the noble gases. 87. Use Table S to compare and look up the properties of specific elements. 88. Energy is rel ...
CHM_101_TUTORIAL_QUESTIONS_1
... decreases the nuclear attraction. This effect is called screening effect but electron-electron repulsion is called shielding effect which also decreases the nuclear attraction. Due to presence of these effects ionisation energy decreases. ...
... decreases the nuclear attraction. This effect is called screening effect but electron-electron repulsion is called shielding effect which also decreases the nuclear attraction. Due to presence of these effects ionisation energy decreases. ...
Chemical bond
A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are ""strong bonds"" such as covalent or ionic bonds and ""weak bonds"" such as Dipole-dipole interaction, the London dispersion force and hydrogen bonding.Since opposite charges attract via a simple electromagnetic force, the negatively charged electrons that are orbiting the nucleus and the positively charged protons in the nucleus attract each other. An electron positioned between two nuclei will be attracted to both of them, and the nuclei will be attracted toward electrons in this position. This attraction constitutes the chemical bond. Due to the matter wave nature of electrons and their smaller mass, they must occupy a much larger amount of volume compared with the nuclei, and this volume occupied by the electrons keeps the atomic nuclei relatively far apart, as compared with the size of the nuclei themselves. This phenomenon limits the distance between nuclei and atoms in a bond.In general, strong chemical bonding is associated with the sharing or transfer of electrons between the participating atoms. The atoms in molecules, crystals, metals and diatomic gases—indeed most of the physical environment around us—are held together by chemical bonds, which dictate the structure and the bulk properties of matter.All bonds can be explained by quantum theory, but, in practice, simplification rules allow chemists to predict the strength, directionality, and polarity of bonds. The octet rule and VSEPR theory are two examples. More sophisticated theories are valence bond theory which includes orbital hybridization and resonance, and the linear combination of atomic orbitals molecular orbital method which includes ligand field theory. Electrostatics are used to describe bond polarities and the effects they have on chemical substances.