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Properties of Metals vs. Nonmetals vs. Metalloids
... Alkali metals, Alkaline Earth metals, Halogens, Noble Gases ...
... Alkali metals, Alkaline Earth metals, Halogens, Noble Gases ...
Midterm Exam 2
... 2) (10 points) In a particular photoelectron spectrum using 22.00 eV photons, electrons were ejected with kinetic energies of 10.00 eV, 8.25 eV, and 5.50 eV. Sketch an energy level diagram for the species, showing the ionization energies of the three identifiable ...
... 2) (10 points) In a particular photoelectron spectrum using 22.00 eV photons, electrons were ejected with kinetic energies of 10.00 eV, 8.25 eV, and 5.50 eV. Sketch an energy level diagram for the species, showing the ionization energies of the three identifiable ...
Study Guide Matter: Building Blocks of the Universe
... * Know the key people in the history of the atom and their contribution to our understanding of the atom. These should be in your lab book conclusion for shoe box atoms. * Know the atomic particles: electron, neutron, and proton. where are they in the atom? What is their charge? What is their mass? ...
... * Know the key people in the history of the atom and their contribution to our understanding of the atom. These should be in your lab book conclusion for shoe box atoms. * Know the atomic particles: electron, neutron, and proton. where are they in the atom? What is their charge? What is their mass? ...
Chem 1411 Chapt2
... Types of CompoundsIonic- Consists of metals and non-metals (Or in general cations and anions). NaCl, MgCl2, K2S, Na2SO4 Molecular (covalent)- Consists of non-metals only. HCl, N2O4, C3H6O, C6H12O6 Note- All compounds can be molecules; not all molecules can be compounds. Ions- Are chemical species th ...
... Types of CompoundsIonic- Consists of metals and non-metals (Or in general cations and anions). NaCl, MgCl2, K2S, Na2SO4 Molecular (covalent)- Consists of non-metals only. HCl, N2O4, C3H6O, C6H12O6 Note- All compounds can be molecules; not all molecules can be compounds. Ions- Are chemical species th ...
Gr 10 Review sheet chemistry
... 1. Change of________________ 2. Formation of a ________________ 3. Formation of _____________ 4. Release or absorption of_____________ ...
... 1. Change of________________ 2. Formation of a ________________ 3. Formation of _____________ 4. Release or absorption of_____________ ...
希臘 - 中正大學化生系
... chemical properties; as is apparent among other series in that of Li, Be, B, C, N, O, and F. 4. The magnitude of the atomic weight determines the character of the element, just as the magnitude of the molecule determines the character of a compound body. 5. We must expect the discovery of many yet u ...
... chemical properties; as is apparent among other series in that of Li, Be, B, C, N, O, and F. 4. The magnitude of the atomic weight determines the character of the element, just as the magnitude of the molecule determines the character of a compound body. 5. We must expect the discovery of many yet u ...
29.2 Chemical Bonds
... When substances are dissolved in water they divide into two categories called acids and bases. An acid creates a sour taste and can dissolve reactive metals like zinc. Vinegar and lemon juice are examples of acids. A base creates a bitter taste and tends to feel slippery. Ammonia is an example ...
... When substances are dissolved in water they divide into two categories called acids and bases. An acid creates a sour taste and can dissolve reactive metals like zinc. Vinegar and lemon juice are examples of acids. A base creates a bitter taste and tends to feel slippery. Ammonia is an example ...
CHM 130 Final Exam Review Chapter 1 Scientific method Theory
... Chemical vs physical properties Chemical vs physical changes Conservation of mass and energy Chapter 5 Models of the atom Atomic notation Isotopes Radiant energy spectrum Wavelength, frequency, energy Levels, sublevels, orbitals Electron configuration Chapter 6 Group names Atomic size trend Metallic ...
... Chemical vs physical properties Chemical vs physical changes Conservation of mass and energy Chapter 5 Models of the atom Atomic notation Isotopes Radiant energy spectrum Wavelength, frequency, energy Levels, sublevels, orbitals Electron configuration Chapter 6 Group names Atomic size trend Metallic ...
A Student want to prepare 250mL of .10 M NaCl solution
... Calculations: you may need to do weighted averages. 20% of a sample is 32grams/mol and 80% 28grams/mol what is the average? ...
... Calculations: you may need to do weighted averages. 20% of a sample is 32grams/mol and 80% 28grams/mol what is the average? ...
投影片 - 中正大學化生系
... chemical properties; as is apparent among other series in that of Li, Be, B, C, N, O, and F. 4. The magnitude of the atomic weight determines the character of the element, just as the magnitude of the molecule determines the character of a compound body. 5. We must expect the discovery of many yet u ...
... chemical properties; as is apparent among other series in that of Li, Be, B, C, N, O, and F. 4. The magnitude of the atomic weight determines the character of the element, just as the magnitude of the molecule determines the character of a compound body. 5. We must expect the discovery of many yet u ...
Easy explanation
... Rutherford conducts gold foil experiment in 1911 • Directed high-energy, positively-charged alpha particles (helium ions from radon) at gold foil surrounded by cylindrical detector • Thomson’s model = no massive concentration of positive charge = nothing to significantly deflect ions • Results: • Mo ...
... Rutherford conducts gold foil experiment in 1911 • Directed high-energy, positively-charged alpha particles (helium ions from radon) at gold foil surrounded by cylindrical detector • Thomson’s model = no massive concentration of positive charge = nothing to significantly deflect ions • Results: • Mo ...
Biol 1406 notes Ch 2 8thed
... electron pair equally and they form a polar covalent bond. o The bonds between oxygen and hydrogen in water are polar covalent because oxygen has a much higher electronegativity than does hydrogen. o Compounds with a polar covalent bond have regions of partial negative charge near the strongly elect ...
... electron pair equally and they form a polar covalent bond. o The bonds between oxygen and hydrogen in water are polar covalent because oxygen has a much higher electronegativity than does hydrogen. o Compounds with a polar covalent bond have regions of partial negative charge near the strongly elect ...
Polarity of Molecules
... polarities of molecules – these will have a major influence on physical properties of substances…… ...
... polarities of molecules – these will have a major influence on physical properties of substances…… ...
PPT | 187.5 KB - Joint Quantum Institute
... more pertinent now that clocks are closing in on the part-per-1018 level of precision New calculations by PFC-supported work at the Joint Quantum Institute and the University of Delaware is the best yet since it includes the most complete treatment of the electron-electron correlations within the Yb ...
... more pertinent now that clocks are closing in on the part-per-1018 level of precision New calculations by PFC-supported work at the Joint Quantum Institute and the University of Delaware is the best yet since it includes the most complete treatment of the electron-electron correlations within the Yb ...
Unit 2: Biochem Notes
... Ionic bonds - One atom loses or donates an electron (becoming a cation/+) and the other atom accepts or gains an electron (becoming an anion/-). As opposite charges attract, they form an ionic bond. ...
... Ionic bonds - One atom loses or donates an electron (becoming a cation/+) and the other atom accepts or gains an electron (becoming an anion/-). As opposite charges attract, they form an ionic bond. ...
Chapter 8 - Power Point Presentation
... • The four regions of high electron density surrounding the oxygen tend to arrange themselves as far from each other as possible in order to minimize repulsive forces. This results in a tetrahedral geometry in which the H-O-H bond angle would be 109.5°. However, the two lone pairs around the oxygen ...
... • The four regions of high electron density surrounding the oxygen tend to arrange themselves as far from each other as possible in order to minimize repulsive forces. This results in a tetrahedral geometry in which the H-O-H bond angle would be 109.5°. However, the two lone pairs around the oxygen ...
Electron configuration Jeopardy
... 500 – What is the difference between a continuous spectrum and a line spectrum and give an example of where you could find each. Continuous spectrum is like the rainbow. You could look out the window to see that. Line spectrum is certain colors show up in lines. You could pass electricity through an ...
... 500 – What is the difference between a continuous spectrum and a line spectrum and give an example of where you could find each. Continuous spectrum is like the rainbow. You could look out the window to see that. Line spectrum is certain colors show up in lines. You could pass electricity through an ...
Chemistry Outcomes - hrsbstaff.ednet.ns.ca
... Give assumptions of Bohr Model Explain the hydrogen line spectrum in terms of Bohr Model of the atom State two differences between the Bohr model and the quantum mechanical model of the atom Draw an energy level diagram for a given atom Define valence shell and valence electrons Label the sublevels ...
... Give assumptions of Bohr Model Explain the hydrogen line spectrum in terms of Bohr Model of the atom State two differences between the Bohr model and the quantum mechanical model of the atom Draw an energy level diagram for a given atom Define valence shell and valence electrons Label the sublevels ...
Ch. 7 Sections 7.9 and 7.11 Powerpoint
... best thing is to be HALF full (one electron in each orbital in the sublevel) • There are many exceptions, but the most common ones are d4 and d9 For the purposes of this class, we are going to assume that ALL atoms (or ions) that end in d4 or d9 are exceptions to the rule. This may or may not be tru ...
... best thing is to be HALF full (one electron in each orbital in the sublevel) • There are many exceptions, but the most common ones are d4 and d9 For the purposes of this class, we are going to assume that ALL atoms (or ions) that end in d4 or d9 are exceptions to the rule. This may or may not be tru ...
Introduction to Chemistry
... Chapter 7 – Atomic Structure and Periodicity Learning Objectives (from Zumdahl Resource Guide): (3-4 days lecture/discussion) To characterize electromagnetic radiation in terms of wavelength, frequency, and speed. To introduce the concept of quantized energy. To show that light has both wave and par ...
... Chapter 7 – Atomic Structure and Periodicity Learning Objectives (from Zumdahl Resource Guide): (3-4 days lecture/discussion) To characterize electromagnetic radiation in terms of wavelength, frequency, and speed. To introduce the concept of quantized energy. To show that light has both wave and par ...
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.