2. Explain how to determine the formula mass (mole mass) for a compound. Molar mass is the mass (in grams) of one mole of a substance. Using the atomic mass of an element and multiplying it by the conversion factor grams per mole (g/mol), you can calculate the molar mass of that element. First, find the chemical formula for the compound.
Those are the orbitals surrounding the atom where the electrons are. Atoms are made of electrons, protons, and neutrons, and the number of those depends on the element. The amount of electrons and protons depends on the element’s atomic number where the atomic number is equal to the number of protons, which is equal to the
Dalton’s atomic theory contained the following ideas: All atoms of a given element are identical. The atoms of different elements vary in mass and size. Atoms are indestructible. Chemical reactions may result in their rearrangement, but not their creation or destruction. Dalton also outlined a law of multiple proportions, which described how reactants will combine in set ratios.
Explain what is meant by relative atomic mass?- Relative atomic mass is the measure of the mass of an element which consists of the protons and neutrons; it is always the bigger number and has the symbol Ar. An obvious example of this is oxygen has the Ar of 16 yet sodium has the Ar of 23. Explain how relative formula mass is calculated using the periodic table- You need to find the relative atomic mass (M) for each atom but this can only be done when the relative atomic mass have been found, then you add all of the masses in the compound together to find the RFM. Sodium Hydroxide is the example we used within our experiment. Na= 23 O= 16 H= 1 NaOH 23 + 16 + 1 = 40 NaOH Mr= 40 Explain how it is possible to work out amounts of substance
Unit 8 LAB- Photoelectric Effect Created by Young Su Kang Materials: • Google PhET Simulation- photoelectric effect Vocabulary: • Electron volt– a unit of energy that is equal to the energy of an electron that is accelerated by a potential difference of 1 volt • Frequency- the number of times something happens in a given period of time • Intensity- a measure of how much energy passes through a region in a given time • Photoelectric effect- the emission of electrons from the surface of a material when struck by electromagnetic radiation • Photon- the smallest possible amount of light; a quantum of light. • Voltage- a measure of the strength of an electrical field. • Wavelength- the distance between consecutive crests or troughs of a wave • Work function- the minimum energy required to remove an electron from a solid
two different directions to the spin. He also gave the world a rule to dictate how an electron in an atom would behave. Pauli’s exclusion principal states that, “if an electron has a certain set of quantum numbers then no other electron in that atom can have the same set of quantum numbers.” When 1926 came Erwin Schrödinger another Austrian physicist built upon Einstein and Louis de Broglie’s idea of wave particle duality. He developed a mathematical Equation that related the pattern of electrons with that of waves, he gave his wave mechanics the symbol psi . In 1932 James Chadwick discovered a second particle in the nucleus, he fired alpha particles at beryllium and found that neutrons were released.
The computationally predicted various possible conformers are shown in Fig.1. The optimized molecular structure with the numbering of atoms of the title compound is shown in Fig.2. The most optimized structural parameters were also calculated by HF/ B3LYP have depicted in Table 1. Quantum chemical calculation was used for NFN to carry out the optimized geometry with the Gaussian 03W program  using the B3LYP and HF functional [11, 12] supplemented with standard 3-21G* basis set. Density Functional Theory (DFT) can be used to calculate an accurate electronic structure, HOMO and LUMO energies, Mulliken charge of atoms, energetic orbital levels, global hardness, chemical potential and electrophilicity of systems, and finally chemical, physical properties of fullerene and fullerene derivatives.
Sulphur is a yellowish, non-metallic chemical element in the periodic table. It is found in group 6 and period 3. Sulphur is identified by the letter S. Since Sulphur is the 16th Element of the periodic table therefore atomic number is always similar as the proton number which is located in the nucleus and converts the nucleus in to a positive charge as neutron is a neutral charge (+-) so positive (+) plus neutral (+-) equals a positive charge. The atomic mass for sulphur is 32 amu or (Atomic Mass Unit is the international system of units). The melting point of sulphur is 112.8 °C and the boiling point of Sulphur is 444.6 °C.
1.1 Kinetic model To determine the second order reaction rate constant of Acesulfame K with the different transient species studied, two pairs of independent competition kinetics were established for each transient: Acesulfame K with Ibuprofen and Acesulfame K with Atrazine. Assuming the first pair of competition for the hydroxyl radical generated by NaNO3 irradiation is Acesulfame and Ibuprofen (ACE, IBP). Their respective reaction rates are (M s-1): (Eq. 6) (Eq. 7) With k and k’ the second order reaction rates of Ace and IBP with HO•.
These metals have only one electron in their outer shell. This means they are ready to lose that one electron in ionic bonding with other elements. As with all metals, the alkali metals are malleable, ductile, and are good conductors of heat and electricity. The alkali metals are softer than most other metals. Cesium and francium are the most reactive elements in this group.