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Table of Contents - Free Coursework for GCSE, IGCSE, A Level, IB
... When it passes through a prism a continuous spectrum is obtained. When energy is applied to specific (individual) elements they emit a spectrum which only contains emissions of particular s. A line spectrum is not continuous. Each element has its own characteristic line spectrum. Hydrogen spectrum ...
... When it passes through a prism a continuous spectrum is obtained. When energy is applied to specific (individual) elements they emit a spectrum which only contains emissions of particular s. A line spectrum is not continuous. Each element has its own characteristic line spectrum. Hydrogen spectrum ...
Atomic Theory
... When it passes through a prism a continuous spectrum is obtained. When energy is applied to specific (individual) elements they emit a spectrum which only contains emissions of particular s. A line spectrum is not continuous. Each element has its own characteristic line spectrum. Hydrogen spectrum ...
... When it passes through a prism a continuous spectrum is obtained. When energy is applied to specific (individual) elements they emit a spectrum which only contains emissions of particular s. A line spectrum is not continuous. Each element has its own characteristic line spectrum. Hydrogen spectrum ...
Practice Exam 3 - University of Missouri
... 7. The thermochemical equation which defines the enthalpy of formation of acetylene, C2H2(g) is a. 2 C(s) + H2(g) → C2H2(g) b. 2 C(g) + 2H(g) → C2H2(g) c. 2 C2(g) + 2H(g) → C2H2(g) d. C2H6(g) → C2H2(g) + H2 e. none of the above 8. Which of the following has a standard molar enthalpy of formation of ...
... 7. The thermochemical equation which defines the enthalpy of formation of acetylene, C2H2(g) is a. 2 C(s) + H2(g) → C2H2(g) b. 2 C(g) + 2H(g) → C2H2(g) c. 2 C2(g) + 2H(g) → C2H2(g) d. C2H6(g) → C2H2(g) + H2 e. none of the above 8. Which of the following has a standard molar enthalpy of formation of ...
Molecules and formulae - Deans Community High School
... The prefix tells us more about the chemical but does not change the elements that are in it. For example carbon tetrachloride is the same as carbon chloride so it will still contain carbon and chlorine; carbon dioxide will still contain carbon and oxygen. Write a heading and try the work below. 1. H ...
... The prefix tells us more about the chemical but does not change the elements that are in it. For example carbon tetrachloride is the same as carbon chloride so it will still contain carbon and chlorine; carbon dioxide will still contain carbon and oxygen. Write a heading and try the work below. 1. H ...
Chapter 4
... Bohr Model of the Hydrogen Atom • Described electrons as PARTICLES – 1913 – Danish physicist – Niels Bohr – Single e- circled around nucleus in allowed paths or orbits – e- has fixed E when in this orbit (lowest E closest to nucleus) – Lot of empty space between nucleus and e- in which e- cannot be ...
... Bohr Model of the Hydrogen Atom • Described electrons as PARTICLES – 1913 – Danish physicist – Niels Bohr – Single e- circled around nucleus in allowed paths or orbits – e- has fixed E when in this orbit (lowest E closest to nucleus) – Lot of empty space between nucleus and e- in which e- cannot be ...
Details
... Structure of the atom, the early atomic theories, theories of electromagnetic radiation, Plank theory, Bohr theory. Quantum theory, Schrodinger wave equation, quantum numbers, shapes of orbitals and electronic configuration. ...
... Structure of the atom, the early atomic theories, theories of electromagnetic radiation, Plank theory, Bohr theory. Quantum theory, Schrodinger wave equation, quantum numbers, shapes of orbitals and electronic configuration. ...
Document
... • A molecule forms when electrons of several atoms interact to form chemical bonds. – The number of bonds an atom can form is determined by the number of valence electrons. • Hydrogen has one electron; it needs one more to fill the inner shell so that it can form one bond. • Carbon has 6 electrons; ...
... • A molecule forms when electrons of several atoms interact to form chemical bonds. – The number of bonds an atom can form is determined by the number of valence electrons. • Hydrogen has one electron; it needs one more to fill the inner shell so that it can form one bond. • Carbon has 6 electrons; ...
Evolution of Atomic Models
... •Quantum- amount of energy required to move an electron from it’s present energy level -Energy is lost and gained -Not always the same (depends on energy level -higher energy level = less distance between energy levels thus less energy is required to move from one level to the next -lower energy le ...
... •Quantum- amount of energy required to move an electron from it’s present energy level -Energy is lost and gained -Not always the same (depends on energy level -higher energy level = less distance between energy levels thus less energy is required to move from one level to the next -lower energy le ...
9. Balancing Equations
... How many sodiums on the left? 2; how many on the right/ 1; put a coefficient 2 in front of the one on the right. How many oxygens on the left/ on the right/, etc. Na2O + BaCl2 - 2NaCl + BaO ...
... How many sodiums on the left? 2; how many on the right/ 1; put a coefficient 2 in front of the one on the right. How many oxygens on the left/ on the right/, etc. Na2O + BaCl2 - 2NaCl + BaO ...
Chapter 5 PPT/Notes B
... λ = 1.37 Å Answer: The wavelength of an electron moving 5.31 x 10 6 m/sec is 1.37 x 10 -10 m or 1.37 Å. ...
... λ = 1.37 Å Answer: The wavelength of an electron moving 5.31 x 10 6 m/sec is 1.37 x 10 -10 m or 1.37 Å. ...
matter and its reactivity. Objects in the universe are composed of
... 3.3a All matter is made up of atoms. Atoms are far too small to see with a light microscope. 3.3c Atoms may join together in well-defined molecules or may be arranged in regular geometric patterns. 3.3d Interactions among atoms and/or molecules result in chemical reactions. 3.3e The atoms of any on ...
... 3.3a All matter is made up of atoms. Atoms are far too small to see with a light microscope. 3.3c Atoms may join together in well-defined molecules or may be arranged in regular geometric patterns. 3.3d Interactions among atoms and/or molecules result in chemical reactions. 3.3e The atoms of any on ...
The valence bond
... Experimentally, the bond dissociation energy, U, for H2 is 458 kJ/mol and for [H2]+ is 269 kJ mol1. experimentally determined bond lengths of H2 and [H2]+ are 74 and 105 pm. ...
... Experimentally, the bond dissociation energy, U, for H2 is 458 kJ/mol and for [H2]+ is 269 kJ mol1. experimentally determined bond lengths of H2 and [H2]+ are 74 and 105 pm. ...
Chp 5 Guided Reading Notes and Vocabulary
... 9. Circle the letter of the formula for the maximum number of electrons that can occupy a principle energy level? Use n for the principle quantum number. a. 2n2 b. n2 c. 2n d. n 5.2 Electron Arrangement in Atoms ...
... 9. Circle the letter of the formula for the maximum number of electrons that can occupy a principle energy level? Use n for the principle quantum number. a. 2n2 b. n2 c. 2n d. n 5.2 Electron Arrangement in Atoms ...
FINAL EXAM REVIEW
... 4. With respect to electrons, how does an ionic bond differ from a covalent bond? 5. Indicate whether the following compounds are ionic, nonpolar covalent, or polar covalent. Explain. a) NaCl b) H2O c) NO2 d) CS2 6. How many valence electrons are there in: a) Si b) K+1 c) Ne ...
... 4. With respect to electrons, how does an ionic bond differ from a covalent bond? 5. Indicate whether the following compounds are ionic, nonpolar covalent, or polar covalent. Explain. a) NaCl b) H2O c) NO2 d) CS2 6. How many valence electrons are there in: a) Si b) K+1 c) Ne ...
Study Guide
... Know the following terms: aggregate, bond angle, covalent bond, delocalized electron, dipole, hybridization, inductive dipole, ionic bond, lattice, Lewis diagram, London Dispersion Force (LDF), orbital, polar, pseudocovalent, quanta, sub-shell, VSEPR, solubility, unsymmetrical, valence and van der W ...
... Know the following terms: aggregate, bond angle, covalent bond, delocalized electron, dipole, hybridization, inductive dipole, ionic bond, lattice, Lewis diagram, London Dispersion Force (LDF), orbital, polar, pseudocovalent, quanta, sub-shell, VSEPR, solubility, unsymmetrical, valence and van der W ...
Matter is made of atoms The atom of each element is characterized
... The spectral lines can be resolved with a prism or a diffraction grating. Multi-electron atoms are complicated. Rules to be learned about later limit the number of electrons in any one state. Thus the electrons in an atom are arranged in concentric shells. The shells are labelled K, L, M, N, etc., s ...
... The spectral lines can be resolved with a prism or a diffraction grating. Multi-electron atoms are complicated. Rules to be learned about later limit the number of electrons in any one state. Thus the electrons in an atom are arranged in concentric shells. The shells are labelled K, L, M, N, etc., s ...
Semester 1 Study Guide – Chemistry
... meaning that only certain discrete energy levels are allowed. ...
... meaning that only certain discrete energy levels are allowed. ...
CH160: Professor Peter Sadler Introduction to inorganic chemistry
... - some alpha particles (He2+, helium nuclei) deflected through angles much larger than 90o; some scattered back toward the source. - Rutherford concluded that atoms contain a verysmall (compared with size of the atom) positive charge, which can repel alpha particles if comes close enough 1911 Ruther ...
... - some alpha particles (He2+, helium nuclei) deflected through angles much larger than 90o; some scattered back toward the source. - Rutherford concluded that atoms contain a verysmall (compared with size of the atom) positive charge, which can repel alpha particles if comes close enough 1911 Ruther ...
4.quantumorbitals
... Quantum Theory The electron is like a cloud of negative energy or a wave. Orbitals are areas in 3D space where the electrons most probably are. The energy of the electron is in its vibrational modes- like notes on a guitar string. Photons are produced when high energy modes change to lower energy mo ...
... Quantum Theory The electron is like a cloud of negative energy or a wave. Orbitals are areas in 3D space where the electrons most probably are. The energy of the electron is in its vibrational modes- like notes on a guitar string. Photons are produced when high energy modes change to lower energy mo ...
S294 Are you Ready for S294 e1i1 web029856
... Metals such as sodium (Na), calcium (Ca), magnesium (Mg) and iron (Fe) may form ionic bonds with other atoms by transferring bonding electrons, and so themselves become positively charged ions. The atoms of the element to which the metal transfers electrons become negatively charged ions, and the r ...
... Metals such as sodium (Na), calcium (Ca), magnesium (Mg) and iron (Fe) may form ionic bonds with other atoms by transferring bonding electrons, and so themselves become positively charged ions. The atoms of the element to which the metal transfers electrons become negatively charged ions, and the r ...
Matter and Its Changes
... Two liquids that don’t mix and stay mixed. They may make a suspension, but they don’t make a ...
... Two liquids that don’t mix and stay mixed. They may make a suspension, but they don’t make a ...
Modules to examine on the Arrangement of Electrons in Atoms website
... Modules to examine on the Arrangement of Electrons in Atoms website: (click to go directly to the different modules) EM Waves Evidence for EM Waves Catch the Wave Stadium Wave Electric Force Quantum Atom Spectral Lines Edvidence for Spectra Absorption Spectra Bohr's Atom Vibrating Charges rev. Adv B ...
... Modules to examine on the Arrangement of Electrons in Atoms website: (click to go directly to the different modules) EM Waves Evidence for EM Waves Catch the Wave Stadium Wave Electric Force Quantum Atom Spectral Lines Edvidence for Spectra Absorption Spectra Bohr's Atom Vibrating Charges rev. Adv B ...
Electrophilic Additions to Double Bonds
... Valence Bond Theory vs. Molecular Orbital Theory For Polyatomic Molecules: Valence Bond Theory: Similar to drawing Lewis structures. Orbitals for bonds are localized between the two bonded atoms, or as a lone pair of electrons on one atom. The electrons in the lone pair or bond do NOT spread out ove ...
... Valence Bond Theory vs. Molecular Orbital Theory For Polyatomic Molecules: Valence Bond Theory: Similar to drawing Lewis structures. Orbitals for bonds are localized between the two bonded atoms, or as a lone pair of electrons on one atom. The electrons in the lone pair or bond do NOT spread out ove ...
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.