Monday, Mar. 23, 2015
... Importance of Bohr’s Model • Demonstrated the need for Plank’s constant in understanding the atomic structure • Assumption of quantized angular momentum which led to quantization of other quantities, r, v and E as ...
... Importance of Bohr’s Model • Demonstrated the need for Plank’s constant in understanding the atomic structure • Assumption of quantized angular momentum which led to quantization of other quantities, r, v and E as ...
111.70 + 48 = 159.70 g/mol
... CALCULATE THE MOLAR MASS OF CARBON DIOXIDE, CO2 The atomic mass of C = 12.01 The atomic mass of O = 16.00 The molar mass of CO2 = 12.01 g/mol + 2(16.00 g/mol) = 12.01+ 32 = 44.01 g/mol http://www.slideshare.net/robertgist/mole-calculations-aeg3 - GOOD REF. ...
... CALCULATE THE MOLAR MASS OF CARBON DIOXIDE, CO2 The atomic mass of C = 12.01 The atomic mass of O = 16.00 The molar mass of CO2 = 12.01 g/mol + 2(16.00 g/mol) = 12.01+ 32 = 44.01 g/mol http://www.slideshare.net/robertgist/mole-calculations-aeg3 - GOOD REF. ...
Slide 1
... then they must all have a sign opposite that of the first particle. 3. If there are other charges nearby, then they must all have a sign the same as that of the first particle. 4. If there are other charges nearby, there must be precisely the same number of positive charges as there are negative cha ...
... then they must all have a sign opposite that of the first particle. 3. If there are other charges nearby, then they must all have a sign the same as that of the first particle. 4. If there are other charges nearby, there must be precisely the same number of positive charges as there are negative cha ...
Document
... how many of a certain type of atom are in a molecule. The bigger number is called the coefficient and tells how many of a particular type of molecule there are. If there is a coefficient in front of the molecule and a subscript after an atom, multiply the coefficient and the subscript to get the num ...
... how many of a certain type of atom are in a molecule. The bigger number is called the coefficient and tells how many of a particular type of molecule there are. If there is a coefficient in front of the molecule and a subscript after an atom, multiply the coefficient and the subscript to get the num ...
Nucleon number
... Matter is anything that has mass and occupies space. All matters consist of tiny particles called atoms. 3 states of matter are solid, liquid and gas. For examples are metal, plastics, gas, etc. ...
... Matter is anything that has mass and occupies space. All matters consist of tiny particles called atoms. 3 states of matter are solid, liquid and gas. For examples are metal, plastics, gas, etc. ...
File
... 65. The volume of 400 mL of chlorine gas at 400mmHg is decreased to 200mL at constant temperature. What is the new gas pressure? A. 400 mmHg B. 300 mmHg C. 800 mmHg D. 650 mmHg 66. If a sealed bag of chips is left in a hot car, what happens to the volume of bag? A. volume increases B. volume decreas ...
... 65. The volume of 400 mL of chlorine gas at 400mmHg is decreased to 200mL at constant temperature. What is the new gas pressure? A. 400 mmHg B. 300 mmHg C. 800 mmHg D. 650 mmHg 66. If a sealed bag of chips is left in a hot car, what happens to the volume of bag? A. volume increases B. volume decreas ...
Movement of Charged Particles
... unit of energy Definition: One electron volt is the energy gained by a particle having a charge of one elementary charge and is accelerated through a 1.0 V potential difference. 1.00 eV = 1.60 x 10-19 J (see data sheet) ...
... unit of energy Definition: One electron volt is the energy gained by a particle having a charge of one elementary charge and is accelerated through a 1.0 V potential difference. 1.00 eV = 1.60 x 10-19 J (see data sheet) ...
Chapter 5: QUANTUM THEORY AND THE ATOM
... Remember that the atomic emission spectra for hydrogen is ___________________________. It is made up of certain ___________________________ of _________________________. Scientists wanted to know _________ this was. In _____________ a Danish physicist named _________________________ came up with a m ...
... Remember that the atomic emission spectra for hydrogen is ___________________________. It is made up of certain ___________________________ of _________________________. Scientists wanted to know _________ this was. In _____________ a Danish physicist named _________________________ came up with a m ...
water, h2o
... The Grotthuss mechanism in a hydrogen-bonded chain, showing the distinct “hop” and “turn” phases It seems especially remarkable, today, that this proposal was made prior to the normally cited date for the atomic theory of matter – clearly the pressure to publish was different in those days! - and b ...
... The Grotthuss mechanism in a hydrogen-bonded chain, showing the distinct “hop” and “turn” phases It seems especially remarkable, today, that this proposal was made prior to the normally cited date for the atomic theory of matter – clearly the pressure to publish was different in those days! - and b ...
Atomic Physics
... A hydrogen atom emits a photon of wavelength 657.7 nm. From what energy state to what lower energy state did the electron jump? ...
... A hydrogen atom emits a photon of wavelength 657.7 nm. From what energy state to what lower energy state did the electron jump? ...
SPECIAL
... began with Rutherford's nuclear model of the atom, with the behavior of the negative electron in the hydrogen atom a small, massive, positively charged nucleus orbited by is at least correctly described by the equation of a circular electronsof mass m and charge-e. Noting that classical non-radiatin ...
... began with Rutherford's nuclear model of the atom, with the behavior of the negative electron in the hydrogen atom a small, massive, positively charged nucleus orbited by is at least correctly described by the equation of a circular electronsof mass m and charge-e. Noting that classical non-radiatin ...
Unit G495 - Field and particle pictures - Insert
... Substituting data quoted earlier in the passage into Equation 7, Box 1, τ is shown to be about 10–14 s. The drift speed of the electron, u, typically 10–3 m s–1, is superimposed on its much higher, random thermal speed, 105 m s–1. This is a similar notion to that of considering the speed of an air p ...
... Substituting data quoted earlier in the passage into Equation 7, Box 1, τ is shown to be about 10–14 s. The drift speed of the electron, u, typically 10–3 m s–1, is superimposed on its much higher, random thermal speed, 105 m s–1. This is a similar notion to that of considering the speed of an air p ...
Department of Physical Sciences (Physics)
... (ii) Explain the deficiencies of the Rutherford model which in turn made it necessary to replace it with the Bohr model listing the main postulates on which the Bohr model is based. Explain why both models apply to atoms with only one electron or to atoms which effectively only have one electron. [6 ...
... (ii) Explain the deficiencies of the Rutherford model which in turn made it necessary to replace it with the Bohr model listing the main postulates on which the Bohr model is based. Explain why both models apply to atoms with only one electron or to atoms which effectively only have one electron. [6 ...
Quantum Mechanics
... treated as continuous variables, Again, this assumption is built into the structure of classical mechanics. ...
... treated as continuous variables, Again, this assumption is built into the structure of classical mechanics. ...
HW Wk9 Solutions
... The total angular momentum of a hydrogen atom in a certain excited state has the quantum number j=3/2. What can you say about the possible values of the orbital angular momentum quantum number l? Solution: The total angular momentum quantum number j is given by j = l ± 12 , and hence l = 2 or l = 1 ...
... The total angular momentum of a hydrogen atom in a certain excited state has the quantum number j=3/2. What can you say about the possible values of the orbital angular momentum quantum number l? Solution: The total angular momentum quantum number j is given by j = l ± 12 , and hence l = 2 or l = 1 ...
Atomic theory
In chemistry and physics, atomic theory is a scientific theory of the nature of matter, which states that matter is composed of discrete units called atoms. It began as a philosophical concept in ancient Greece and entered the scientific mainstream in the early 19th century when discoveries in the field of chemistry showed that matter did indeed behave as if it were made up of atoms.The word atom comes from the Ancient Greek adjective atomos, meaning ""uncuttable"". 19th century chemists began using the term in connection with the growing number of irreducible chemical elements. While seemingly apropos, around the turn of the 20th century, through various experiments with electromagnetism and radioactivity, physicists discovered that the so-called ""uncuttable atom"" was actually a conglomerate of various subatomic particles (chiefly, electrons, protons and neutrons) which can exist separately from each other. In fact, in certain extreme environments, such as neutron stars, extreme temperature and pressure prevents atoms from existing at all. Since atoms were found to be divisible, physicists later invented the term ""elementary particles"" to describe the ""uncuttable"", though not indestructible, parts of an atom. The field of science which studies subatomic particles is particle physics, and it is in this field that physicists hope to discover the true fundamental nature of matter.