solving atomic calculations: working with: – elements – isotopes – ions – atomic # –...
TRANSCRIPT
Solving atomic calculations:
• Working with:– Elements– Isotopes– Ions
– Atomic #– Atomic mass– Charge
THE BASICS:Elements, Isotopes, and Ions
1. ELEMENTS: are atoms with the same # of protons (same Atomic #)
2. ISOTOPES (mass): are atoms of the same element with a particular # of neutrons (electrons aren’t involved)
3. IONS (charge): are atoms of the same element with a particular # of electrons (neutrons aren’t involved)
Elements, Isotopes, and IonsREMEMBER:-protons:
-have a charge of +1, so they are involved in determining ions
(atoms of a particular charge)-have a mass of 1, so they
are involved in determining isotopes (atoms of a particular mass)
REMEMBER:
-neutrons:
-have a charge of 0, so they are NOT involved in determining ions
(atoms of a particular charge)
-have a mass of 1, so they are involved in determining isotopes (atoms of a particular mass)
REMEMBER:
-electrons:
-have a charge of -1, so they are involved in determining ions (atoms of a particular charge)
-have a mass of almost 0, so they are
NOT involved in determining isotopes(atoms of a particular mass)
CALCULATIONS• MASS NUMBER: – Is the total mass of a certain ISOTOPE of an
element.
1. How to calculate mass #:# of protons + # of neutrons = mass #
2. How to calculate # of neutrons from mass #:
(Mass #) – (atomic #) = # of neutrons
↕ ↕ ↕ (# of P + # of N) – (# of P) = # of N
CALCULATIONS• CHARGE, OR IONS: – Is the total charge (+ or - ) of a certain ION of an
element.
1. How to calculate charge:Difference between the # of protons & # of electrons =
charge of an ion
2. How to calculate # of neutrons from mass #:(+ Protons ) + (- electrons) = chargeEx.: +5p + (-3e) = +2 OR
+ 5 p - -3e = 2, since there’s more p’s than e’s, its +2
CALCULATIONS:• ATOMIC # FROM OTHER INFORMATION:
1. From the charge:Ex.: if an atom has a charge of +2, and has 6- electrons, its Atomic # = 8 (+2 means it has 2 more + protons than
-electrons; (+2) + (6 electrons) = 8 protons = atomic # 8)
2. from # of neutrons and the mass #:(Mass #) – (# of neutrons) = atomic #
↕ ↕ ↕ (# of P + # of N) – (# of neutrons) = (# of P)