what is the relation between atomic weight equivalent weight and valency?
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The equivalent weight of an element or radical is equal to its atomic weight or formula weight divided by the valence it assumes in compounds. The unit of equivalent weight is the atomic mass unit ; the amount of a substance in grams numerically equal to the equivalent weight is called a gram equivalent.
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Relative molecular mass is the sum of the atomic masses of the atoms in the molecule. Relative formula mass is the sum of the atomic masses of the atoms in the empirical formula(Atomic subscripts reduced to their lowest terms).
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The main difference between valency and covalency is that valency is the number of electrons that an atom will lose or gain in order to stabilize itself whereas covalency is the maximum number of covalent bonds that an atom can form using its empty orbitals.
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Equivalent weights may be calculated from molar masses if the chemistry of the substance is well known: sulfuric acid has a molar mass of 98.078(5) g mol−1, and supplies two moles of hydrogen ions per mole of sulfuric acid, so its equivalent weight is 98.078(5) g mol−1/2 eq mol−1 = 49.039(3) g eq−1.
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Atomic weight: The sum of mass number of proton and mass number of neutron is called atomic weight or atomic mass number (A). Z = 19 and A = 39 as per atomic weight definition. Isotopes: Atoms of the same element contains different number of neutrons, are called isotopes.
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Elements in the same group have the same number of valence electrons and so interact with other elements in a similar way. They display similar physical and chemical properties. For example, the halogens (F, Cl, Br, I) all react similarly.
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Electron affinity is directly proportional to atomic radius. Intuitively speaking, the valence electrons which are close to the nucleus will experience a greater influence of the nucleus. Similarly the incoming electron will lose greater amount of energy in case it is closer to the nucleus.
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For groups 1-2 and 13-18, the valency is directly related to group number. So, elements in group one, the alkali metals, have one valence electron, those in group two have two valence, those in group thirteen have three electrons, and so on.
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charge is always related to atoms whereas valency is related to elements and is similar to the number of ion (negative or positive) present on the element. VALENCY IS A COMBINING CAPACITY OF AN ELEMENT.
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Equivalent weight (also known as gram equivalent) is the mass of one equivalent, that is the mass of a given substance which will combine with or displace a fixed quantity of another substance.
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The valency and oxidation state may have the same values or different values. Valency is the number of electrons present in the outermost shell of a particular element whereas oxidation state is the number of electrons that an element in a particular compound has lost or gained.
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Ex: The molecular mass of oxygen is 32. This means that oxygen is 32 times heavier than 1/12th of the mass of carbon 12. Equivalent mass is defined as the number of parts by mass of the substance which combine or displace 1.008 parts by mass of hydrogen or 8 parts by mass of oxygen or 35.5 parts by mass of chlorine.
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The formula mass (formula weight) of a molecule is the sum of the atomic weights of the atoms in its empirical formula. The molecular mass (molecular weight) of a molecule is its average mass as calculated by adding together the atomic weights of the atoms in the molecular formula.
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Atomic mass (ma) is the mass of an atom. A single atom has a set number of protons and neutrons, so the mass is unequivocal (won't change) and is the sum of the number of protons and neutrons in the atom. ... Atomic weight is a weighted average of the mass of all the atoms of an element, based on the abundance of isotopes.
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There is a unique relationship between molar mass and atomic weight: Oxygen's atomic weight is 16.00 amu. 1 mole of oxygen is 6.02 x 1023 atoms of oxygen 1 amu = 1.661 x 10-24g What is the molar mass (g/mole) of oxygen? Molar mass (in grams) is always equal to the atomic weight of the atom!
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What notations are used to represent atomic number and weight? Each atom, therefore, can be assigned both an atomic number (the number of protons equals the number of electrons) and an atomic weight (approximately equaling the number of protons plus the number of neutrons).
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element Percentage Atomic Weight Relative Numberofatoms Simplest Whole Number Ratio C 80 12 80/12 =6.67 6.67/6.67 = 1 H 20 1 20/1 =20 20/6.67 = 3so The Emperical Formula Of The Compound Is CH3the Weight Of This ...