protons are positive (+) charged particles found in the nucleus of an atom
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Chapter 4 - Part 2. Protons , neutrons and electrons are all subatomic particles. Protons are positive (+) charged particles found in the nucleus of an atom. Proton mass = 1.674 x 10 -24 g 1 proton = +1 Charge. Nucleus. Proton. Neutron. Electron. The Neutron - PowerPoint PPT PresentationTRANSCRIPT
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•Protons are positive (+) charged particles found in the nucleus of an atom.
•Proton mass = 1.674 x 10-24g
•1 proton = +1 Charge
•Protons, neutrons and electrons are all subatomic particles.
Chapter 4 - Part 2
NucleusProton
Electron
Neutron
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The Neutron
•The neutron is a subatomic particle found in the nucleus.
•1 neutron = no charge
•The neutron was discovered in 1932 by James Chadwick.
•Its mass is almost the same as a proton.
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The Electron
•The electron is a subatomic particle found outside of the nucleus of an atom and it has a negative (-) charge.
•Electrons mass = 9.11 x 10-28g
•1 electron = -1 charge
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Charge
A proton has a positive charge +1
An electron has a negative charge -1
A neutron is neutral. It won’t affect overall charge.
One positive proton will cancel out one negative electron leaving an overall charge of Zero
0
+1 -1
Overall Charge = 0
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Complete the table below
Atom ChargeProtons
Charge Neutrons
Charge Electrons
Overall Charge
5 protons6 neutrons5 electrons
16 protons16 neutrons16 electrons
19 protons20 neutrons19 electrons
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Elements are organized into rows and columns based on their atomic number.
The Periodic Table
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Hydrogen1.008
1
atomicnumber
chemicalsymbol
name atomicmass
Mercury200.59
80
Elements, symbols and masses
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Atomic Number•Atomic number = # of protons for an element.
•Atoms of different elements has different numbers of protons.
•Each positive charged proton must be balanced by a negative charged electron. So the atomic # lets you know the # of protons and the # of electrons.
•Example: Sulfur (S) is atomic number 16 because it has 16 protons. Since it has 16 protons it has to have 16 electrons.
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Mass Number•The mass number lets you figure out how many neutrons are present in an element.
•Mass # = # of protons + # of neutrons or m=p+n
•Neutrons = mass # - atomic # since the atomic number is the same as the number of protons then n=m-p
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•Example: Aluminum (Al) has 13 protons.
Its mass number is 27.
So, 27-13=14 and 14 is the number of neutrons found in an atom of Aluminum.
Mass number continued…
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Atomic Mass Units
•An atomic mass unit (amu) is defined as 1/12th of a Carbon-12 atom.
•AMU’s is the unit of mass used on the periodic table when looking at an elements atomic mass number.
•That's about the mass of one proton or neutron.
1 AMU
U
Protons and Neutrons = 1 amu each
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•One gram is about 600,000,000,000,000,000,000,000 amu.
•Ex: Fluorine’s (F) atomic mass is 19 amu, but it’s mass in grams is 3.155 x 10 -28 grams.
•Wow--I can see why you'd want to use amu's instead of grams.
AMU’s continued…
•1 atomic mass unit = 1.66053886 × 10-24 kg
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What is the atomic mass of an atom with…
4 protons and 5 neutrons =
24 protons and 28 neutrons =
7 protons and 7 neutrons =
91 protons and 140 neutrons =
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Complete the table below:
Protons Neutrons Atomic Mass
35 65
10 20
39 70
39 89
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Isotopes
•Isotopes are atoms of the same element but have a different number of neutrons and mass number.•Example: Oxygen (O) has 8 protons but some atoms of oxygen have a mass # of 16, 17 or 18.
•So this means the number of neutrons varies between each isotope. So Oxygen-16 has 8 neutrons, Oxygen-17 has 9 neutrons and Oxygen-18 has 10 neutrons.
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Common Isotopes
•The element Carbon (C) can be found as C12, C13 and C14.
•How many protons, neutrons and electrons does each carbon isotope above have?
Answer: C12 – 6,6,6
C13 – 6,7,6
C14 – 6,8,6
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•Hydrogen-1 doesn’t have any neutrons.
•Hydrogen-2 has 1 neutron
•Hydrogen-3 has 2 neutrons
Hydrogen Isotopes