Chapter 2 BIO 100 Chemistry
... Electron Energy Levels: • Electrons = Negatively (-) charged particles that orbit around the nucleus. ...
... Electron Energy Levels: • Electrons = Negatively (-) charged particles that orbit around the nucleus. ...
Covalent Bonding - Effingham County Schools
... •As independent particles, most atoms are at relatively high potential energy. •Nature, however, favors arrangements in which potential energy is minimized. •This means that most atoms are less stable existing by themselves than when they are combined. •By bonding with each other, atoms decrease in ...
... •As independent particles, most atoms are at relatively high potential energy. •Nature, however, favors arrangements in which potential energy is minimized. •This means that most atoms are less stable existing by themselves than when they are combined. •By bonding with each other, atoms decrease in ...
CH8
... 2. Usually expressed as the energy needed to break one mole of bonds. 3. A large bond dissociation energy corresponds to a strong covalent bond. 4. High dissociation energies tend to create very stable compounds that tend to be chemically unreactive. 5. Units are measured in kJ/mo1 6. A mol is a che ...
... 2. Usually expressed as the energy needed to break one mole of bonds. 3. A large bond dissociation energy corresponds to a strong covalent bond. 4. High dissociation energies tend to create very stable compounds that tend to be chemically unreactive. 5. Units are measured in kJ/mo1 6. A mol is a che ...
Exam Review
... d. How is the number of protons determined? From the atomic number e. How is the number of neutrons determined? Mass # - # of protons f. How is the number of electrons determined in a neutral atom? # protons = # electrons g. What subatomic particles are located in the nucleus? Protons and neutrons h ...
... d. How is the number of protons determined? From the atomic number e. How is the number of neutrons determined? Mass # - # of protons f. How is the number of electrons determined in a neutral atom? # protons = # electrons g. What subatomic particles are located in the nucleus? Protons and neutrons h ...
High School Physical Science Glossary
... more particles; in order of decreasing strength: the strong force, the electromagnetic force, the weak force, and gravity gamma radiation- form of radiation emitted from the nucleus in high energy waves; may be blocked by a thick layer of lead gas- state of matter without a definite shape or volume ...
... more particles; in order of decreasing strength: the strong force, the electromagnetic force, the weak force, and gravity gamma radiation- form of radiation emitted from the nucleus in high energy waves; may be blocked by a thick layer of lead gas- state of matter without a definite shape or volume ...
Document
... which is close to, but not exactly equal to, the electron mass. The origin of our coordinate system is now at the center of mass between the electron and proton, which of course will stay quite close to the proton. The key to solving the hydrogen atom is to take advantage of the spherical symmetry, ...
... which is close to, but not exactly equal to, the electron mass. The origin of our coordinate system is now at the center of mass between the electron and proton, which of course will stay quite close to the proton. The key to solving the hydrogen atom is to take advantage of the spherical symmetry, ...
lecture_CH1-2review_chem121pikul
... Distinguish the difference between chemical and physical properties & changes We represent uncertainty with significant figures You do not need to memorize Sig Fig rules Scientific Notation Conversions within the metric system and non metric units Temperature conversions Density & Spec ...
... Distinguish the difference between chemical and physical properties & changes We represent uncertainty with significant figures You do not need to memorize Sig Fig rules Scientific Notation Conversions within the metric system and non metric units Temperature conversions Density & Spec ...
1 eV
... To be consistent with the Heisenberg Uncertainty Principle, which of these properties cannot be quantized (have the exact value known)? (more than one answer can be correct) Electron Radius Electron Energy Electron Velocity Electron Angular Momentum Physics 102: Lecture 24, Slide 22 ...
... To be consistent with the Heisenberg Uncertainty Principle, which of these properties cannot be quantized (have the exact value known)? (more than one answer can be correct) Electron Radius Electron Energy Electron Velocity Electron Angular Momentum Physics 102: Lecture 24, Slide 22 ...
valence electrons
... & position of a particle at the same time. • In order to find position of an electron, need photon of light. • Photon “bumps” into electron, changing its position. ...
... & position of a particle at the same time. • In order to find position of an electron, need photon of light. • Photon “bumps” into electron, changing its position. ...
pages 1-2 of the lecture notes
... J.J. Thomson (English physicist, 1856-1940) in 1897 discovers the electron and determines the charge to mass ratio. In 1906 he wins the Nobel Prize. The Experiment: ...
... J.J. Thomson (English physicist, 1856-1940) in 1897 discovers the electron and determines the charge to mass ratio. In 1906 he wins the Nobel Prize. The Experiment: ...
Chemical Foundations: Elements, Atoms and Ions
... Elements are made of tiny particles called atoms All atoms of a given element are identical Atoms of a given element are different from those of any other element 4. Atoms of one element can combine with atoms of other elements to form compounds 5. Atoms are indivisible and can not be created or des ...
... Elements are made of tiny particles called atoms All atoms of a given element are identical Atoms of a given element are different from those of any other element 4. Atoms of one element can combine with atoms of other elements to form compounds 5. Atoms are indivisible and can not be created or des ...
Lecture 7 - United International College
... atoms • All atoms of a given element are identical • The atoms of a given element are different from those of any other element • Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative numbers of types of atoms. • Atoms cannot b ...
... atoms • All atoms of a given element are identical • The atoms of a given element are different from those of any other element • Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative numbers of types of atoms. • Atoms cannot b ...
PHYS 113: Quantum Mechanics Waves and Interference In much of
... (where the probability is 0, for example), where you’d never find it. One caveat: once you look at the electron or observe it in any way, you will totally change its wave-function. After all, you know where it is! What you’ll find is that, by the uncertainty principle, you now don’t know the momentu ...
... (where the probability is 0, for example), where you’d never find it. One caveat: once you look at the electron or observe it in any way, you will totally change its wave-function. After all, you know where it is! What you’ll find is that, by the uncertainty principle, you now don’t know the momentu ...
WBL6_Lecture_Ch27
... of atom has its own set of wavelengths. An empirical formula was found that gives the four visible spectral lines of hydrogen: ...
... of atom has its own set of wavelengths. An empirical formula was found that gives the four visible spectral lines of hydrogen: ...
Franck-Hertz Experiment – Quantized Energy Levels in Atoms
... The purpose of this experiment is to observe the discrete energy states in neon atoms. As electrons are accelerated through the rarified neon gas they move toward the anode, and sometimes collide with a neon atom. If the accelerated electron has sufficient kinetic energy, its collision with a neon a ...
... The purpose of this experiment is to observe the discrete energy states in neon atoms. As electrons are accelerated through the rarified neon gas they move toward the anode, and sometimes collide with a neon atom. If the accelerated electron has sufficient kinetic energy, its collision with a neon a ...
Atomic orbital
An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus. The term may also refer to the physical region or space where the electron can be calculated to be present, as defined by the particular mathematical form of the orbital.Each orbital in an atom is characterized by a unique set of values of the three quantum numbers n, ℓ, and m, which respectively correspond to the electron's energy, angular momentum, and an angular momentum vector component (the magnetic quantum number). Any orbital can be occupied by a maximum of two electrons, each with its own spin quantum number. The simple names s orbital, p orbital, d orbital and f orbital refer to orbitals with angular momentum quantum number ℓ = 0, 1, 2 and 3 respectively. These names, together with the value of n, are used to describe the electron configurations of atoms. They are derived from the description by early spectroscopists of certain series of alkali metal spectroscopic lines as sharp, principal, diffuse, and fundamental. Orbitals for ℓ > 3 continue alphabetically, omitting j (g, h, i, k, …).Atomic orbitals are the basic building blocks of the atomic orbital model (alternatively known as the electron cloud or wave mechanics model), a modern framework for visualizing the submicroscopic behavior of electrons in matter. In this model the electron cloud of a multi-electron atom may be seen as being built up (in approximation) in an electron configuration that is a product of simpler hydrogen-like atomic orbitals. The repeating periodicity of the blocks of 2, 6, 10, and 14 elements within sections of the periodic table arises naturally from the total number of electrons that occupy a complete set of s, p, d and f atomic orbitals, respectively.