Solving atomic calculations: Working with: – Elements – Isotopes – Ions – Atomic # – Atomic mass – Charge.

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Presentation 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 Ions REMEMBER: -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) = charge Ex.: + 5p + ( - 3e) = +2OR + 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)