Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms...
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Transcript of Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms...
![Page 1: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/1.jpg)
Atomic Number- the number of protons in the nucleus of an atom of that element
Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic number is 1.
Atoms are neutral, so the # of protons =# of electrons.
![Page 2: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/2.jpg)
Total number of protons and neutrons in an atom.
Mass = # protons + # neutrons The # of neutrons in an atom is the
difference between mass # and atomic #. # Neutrons = Mass # - Atomic #
![Page 3: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/3.jpg)
Atoms that have the same # of protons, but different # of neutrons.
If they have more/less neutrons, then the mass number will be different!
Have same number of protons and electrons. Only difference is # of neutrons!
![Page 4: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/4.jpg)
A way to measure the mass of an atom, using a standard (carbon-12).
Carbon-12 has 6 protons and 6 neutrons. It’s mass is set at 12 amu. So the mass of a single proton or neutron is about 1 amu.
Atomic Mass- weighted average mass of the atoms in a naturally occurring sample of the element.
![Page 5: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/5.jpg)
![Page 6: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/6.jpg)
Ca
P-3
Al+3
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1. Change abundance percents into decimals.
2. Multiply the mass of each isotope by its natural abundance. (expressed as decimal)
3. Add the products.
![Page 8: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/8.jpg)
Element X has two natural isotopes. The isotope with a mass of 10.012 amu has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu has a relative abundance of 80.09%. Calculate the atomic mass and identify this element.
![Page 9: Atomic Number- the number of protons in the nucleus of an atom of that element Ex: Hydrogen atoms have only one proton in the nucleus, so the atomic.](https://reader035.fdocuments.in/reader035/viewer/2022070403/56649f305503460f94c4b7ae/html5/thumbnails/9.jpg)
The element copper has naturally occurring isotopes with mass numbers of 63 and 65. The relative abundance and atomic masses are 69.2% for mass = 62.93 amu, and 30.8% for mass = 64.93 amu. Calculate the average atomic mass of copper.
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Calculate the atomic mass of bromine. The two isotopes of bromine have atomic masses and relative abundance of 78.92 amu (50.69%) and 80.92 amu (49.31%).