Atomic mass of ag

Chemical Elements.com - Silver (Ag) Show Table With: Element Groups: Name: Silver Symbol: Ag Atomic Number: 47 Atomic Mass: 107.8682 amu Melting Point: 961.93 °C (1235.08 K, 1763.474 °F) Boiling Point: 2212.0 °C (2485.15 K, 4013.6 °F) Number of Protons/Electrons: 47 Number of Neutrons: 61 Classification: Crystal Structure: Cubic Density @ 293 K: 10.5 g/cm 3 Color: silver Number of Energy Levels: 5 First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 18 Fourth Energy Level: 18 Fifth Energy Level: 1 Isotope Half Life Ag-105 41.3 days Ag-105m 7.2 minutes Ag-106m 8.4 days Ag-107 Stable Ag-108 2.4 minutes Ag-108m 130.0 years Ag-109 Stable Ag-109m 39.8 seconds Ag-110 24.6 seconds Ag-110m 249.8 days Ag-111 7.47 days Date of Discovery: Known to the ancients Discoverer: Unknown Name Origin: From the Old English word seolfor (silver) Symbol Origin: From the Latin word argentum (silver) Uses: jewelry, photography, electrical conductor Obtained From: ores (argentite, light ruby silver, dark ruby silver, brittle silver) Bentor, Yinon. Chemical Element.com - Silver. For more information about citing online sources, please visit the This page was created by Yinon Bentor. Use of this web site is restricted by this site's Copyright © 1996-2012 Yinon Bentor. All Rights Reserved.

Glossary Group A vertical column in the periodic table. Members of a group typically have similar properties and electron configurations in their outer shell. Period A horizontal row in the periodic table. The atomic number of each element increases by one, reading from left to right. Block Elements are organised into blocks by the orbital type in which the outer electrons are found. These blocks are named for the characteristic spectra they produce: sharp (s), principal (p), diffuse (d), and fundamental (f). Atomic number The number of protons in an atom. Electron configuration The arrangements of electrons above the last (closed shell) noble gas. Melting point The temperature at which the solid–liquid phase change occurs. Boiling point The temperature at which the liquid–gas phase change occurs. Sublimation The transition of a substance directly from the solid to the gas phase without passing through a liquid phase. Density (g cm −3) Density is the mass of a substance that would fill 1 cm 3 at room temperature. Relative atomic mass The mass of an atom relative to that of carbon-12. This is approximately the sum of the number of protons and neutrons in the nucleus. Where more than one isotope exists, the value given is the abundance weighted average. Isotopes Atoms of the same element with different numbers of neutrons. CAS number The Chemical Abstracts Service registry number is a unique identifier of a particular chemical, designed to prevent confusion arising from diff...

Skills to Develop • Define the atomic mass unit and average atomic mass • Calculate average atomic mass and isotopic abundance • Define the amount unit mole and the related quantity Avogadro’s number • Explain the relation between mass, moles, and numbers of atoms or molecules, and perform calculations deriving these quantities from one another Isotopes The symbol for a specific isotope of any element is written by placing the mass number as a superscript to the left of the element symbol (Figure \(\PageIndex\) 10 10 12 21.9914 9.25 Use this Build an Atom simulator to build atoms of the first 10 elements, see which isotopes exist, check nuclear stability, and gain experience with isotope symbols. Atomic Mass Because each proton and each neutron contribute approximately one amu to the mass of an atom, and each electron contributes far less, the atomic mass of a single atom is approximately equal to its mass number (a whole number). However, the average masses of atoms of most elements are not whole numbers because most elements exist naturally as mixtures of two or more isotopes. The mass of an element shown in a periodic table or listed in a table of atomic masses is a weighted, average mass of all the isotopes present in a naturally occurring sample of that element. This is equal to the sum of each individual isotope’s mass multiplied by its fractional abundance. \[\mathrm\] It is important to understand that no single boron atom weighs exactly 10.8 amu; 10.8 amu is the a...

\( \newcommand\) • • • • • • • Learning Objectives • Use Avogadro's number to convert to moles and vice versa given the number of particles of an element. • Use the molar mass to convert to grams and vice versa given the number of moles of an element. When objects are very small, it is often inconvenient or inefficient, or even impossible to deal with the objects one at a time. For these reasons, we often deal with very small objects in groups, and have even invented names for various numbers of objects. The most common of these is "dozen" which refers to 12 objects. We frequently buy objects in groups of 12, like doughnuts or pencils. Even smaller objects such as straight pins or staples are usually sold in boxes of 144, or a dozen dozen. A group of 144 is called a "gross". This problem of dealing with things that are too small to operate with as single items also occurs in chemistry. Atoms and molecules are too small to see, let alone to count or measure. Chemists needed to select a group of atoms or molecules that would be convenient to operate with. Avogadro's Number In chemistry, it is impossible to deal with a single atom or molecule because we can't see them or count them or weigh them. Chemists have selected a number of particles with which to work that is convenient. Since molecules are extremely small, you may suspect this number is going to be very large and you are right. The number of particles in this group is \(6.02 \times 10^\) of those objects. There is a ...