Just a Little More Atomic Structure Info

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Presentation transcript:

Just a Little More Atomic Structure Info Ions And Isotopes Just a Little More Atomic Structure Info

What are isotopes Isotopes are atoms of the same element with differing numbers of neutrons Different numbers of neutrons mean a different mass number For example there are two naturally occurring stable forms of Boron One form Boron – 10 has a mass of 10.0 - five neutrons One form Boron -11 has a mass of 11.0 – six neutrons Notice the way to write the isotope; element name with the mass number Each form has 5 protons so it is still boron

More examples Isotope Lithium 6 Nitrogen – 15 Calcium – 44 Argon – 38 Number of neutrons 3 neutrons 8 neutrons 24 neutrons 20 neutrons

Isotope Notation Notation shows elements symbol, mass and atomic number of that isotope This isotope has a mass of 14, means it has how many neutrons? 8 neutrons

Just What Is an Ion An ion is an atom that has lost or gained an electron or electrons Number of protons do not change An ion has a net charge on it. Ions can exist as simple atoms Na+, Cl- Ions can exist as several atoms called polyatomic ions; NO3-, S04-2

How to determine the charge Atoms gain or lose electrons to become charged Electrons have a negative charge So……. If an atom loses electrons it becomes positively charged Sodium,Na loses one electrons to become Na+ Aluminum, loses three electrons to become Al+3 If an atom gains electrons it becomes negatively charged Chlorine, Cl, gains one electron to become Cl- Phosphorus, P, gains three electrons to become P-3

Na+ Ions and Isotopes Mass Number How many protons in this ion? 22 How many neutrons in this ion? 11 How many electrons in this ion? Atomic Number

P-3 Lets Try Again 31 15 How many protons in this ion? How many neutrons in this ion? How many electrons in this ion?

Bi-2 One More Time !! 209 83 How many protons in this ion? How many neutrons in this ion? How many electrons in this ion

A difference in terms Atomic mass – listed on the periodic table for an element based upon the weighted average of the isotopes of that element Mass number – the mass of a particular isotope of that element