Presentation is loading. Please wait.

Presentation is loading. Please wait.

Calculating Average Atomic Mass

Published byCarol Cook Modified over 5 years ago

Similar presentations

Presentation on theme: "Calculating Average Atomic Mass"— Presentation transcript:

1 Calculating Average Atomic Mass
Atomic Structure Calculating Average Atomic Mass

2 Mass of isotope (Relative Atomic Mass)
Average Atomic Mass Weight underneath each element on the periodic table is an average of all the isotopes that exist for that specific element 1 H 1.0079 Hydrogen Isotopes of Hydrogen Mass of isotope (Relative Atomic Mass) Percent Abundance (%) Hydrogen – 1 Hydrogen – 2 0.0115 Hydrogen – 3 0.003

3 Which isotope of Hydrogen is most abundant?
Isotopes of Hydrogen Mass of isotope (Relative Atomic Mass) Percent Abundance (%) Hydrogen – 1 Hydrogen – 2 0.0115 Hydrogen – 3 0.003 The isotope whose mass is closest to the average atomic mass is the most abundant.

4 Which isotope is more abundant given the average atomic mass of
Practice questions Which isotope is more abundant given the average atomic mass of Carbon is , C-14 or C-12?

5 Calculating Average Atomic Mass
Convert Percentages into DECIMALS These percentages are your percent abundance #’s To do this you need to Divide by 100 Multiply the percent abundance DECIMALS by its relative atomic mass Add ALL the numbers from STEP 2 together

6 These percentages are your percent abundance #’s
1. Convert Percentages into DECIMALS These percentages are your percent abundance #’s (Divide by 100) 2. Multiply the percent abundance DECIMALS by its relative atomic mass 3. Add ALL the numbers from STEP 2 together Naturally occurring copper is 69.1% Cu-63 and 30.9% Cu-65. What is the average atomic mass?

7 These percentages are your percent abundance #’s
1. Convert Percentages into DECIMALS These percentages are your percent abundance #’s (Divide by 100) 2. Multiply the percent abundance DECIMALS by its relative atomic mass 3. Add ALL the numbers from STEP 2 together What is the average atomic mass of a sample of Neon with 90.0% Neon-20 & 10.0%Neon-22?

8 These percentages are your percent abundance #’s
1. Convert Percentages into DECIMALS These percentages are your percent abundance #’s (Divide by 100) 2. Multiply the percent abundance DECIMALS by its relative atomic mass 3. Add ALL the numbers from STEP 2 together Calculate the average atomic weight for carbon from the following isotopic information: % Carbon-12 (exact mass 12.00) and 1.108% Carbon-13 (exact mass )

Download ppt "Calculating Average Atomic Mass"

Similar presentations

Average Atomic Mass. How much does an atom weigh?  Protons & Neutrons:  1.67 X 10 -24 gram  Electrons:  9.10 X 10 -28 gram  To avoid working with.

Average Atomic Mass. How much does an atom weigh?  Protons & Neutrons:  1.67 X gram  Electrons:  9.10 X gram  To avoid working with.
Calculating Average Atomic Mass. Introduction The value for atomic mass for a particular element is the average atomic mass. Each sample of an element.

Calculating Average Atomic Mass. Introduction The value for atomic mass for a particular element is the average atomic mass. Each sample of an element.
ISOTOPIC NOTATION isotopes are atoms with the same number of protons but different number of neutrons A Z X A = mass number (the total number of protons.

ISOTOPIC NOTATION isotopes are atoms with the same number of protons but different number of neutrons A Z X A = mass number (the total number of protons.
Average Atomic Mass.

Average Atomic Mass.
Relative atomic mass Atoms are too small to be weighed individually, even with the best balance! We can, however, compare the masses of different atoms.

Relative atomic mass Atoms are too small to be weighed individually, even with the best balance! We can, however, compare the masses of different atoms.
1 Average Atomic Mass Chemistry Notes. 2 Relative Atomic Mass  Masses of atoms expressed in grams are very small, for example: One atom of Oxygen-16.

1 Average Atomic Mass Chemistry Notes. 2 Relative Atomic Mass  Masses of atoms expressed in grams are very small, for example: One atom of Oxygen-16.
Atomic Calculations and Mass Spectrometry Quantum Orbital Video.

Atomic Calculations and Mass Spectrometry Quantum Orbital Video.
 Definition: Atoms of the same element that differ in their # of neutrons; therefore, they have different mass numbers.  Nearly every element has isotopes!

 Definition: Atoms of the same element that differ in their # of neutrons; therefore, they have different mass numbers.  Nearly every element has isotopes!
Average Atomic Mass. Masses of Atoms A scale designed for atoms gives their small atomic masses in atomic mass units (amu) An atom of 12 C was assigned.

Average Atomic Mass. Masses of Atoms A scale designed for atoms gives their small atomic masses in atomic mass units (amu) An atom of 12 C was assigned.
 Each element on the periodic table has an isotope.  What make an element have different isotopes?  There are 2 different isotopes of iron  Find the.

 Each element on the periodic table has an isotope.  What make an element have different isotopes?  There are 2 different isotopes of iron  Find the.
Average Atomic Mass. Average Atomic Mass – the weighted average of the masses of the isotopes of an element Every element is composed of several naturally.

Average Atomic Mass. Average Atomic Mass – the weighted average of the masses of the isotopes of an element Every element is composed of several naturally.
Atomic Mass. Isotopes Reminder Yesterday we learned that the mass of all atoms of a certain element are not always the same –Some atoms may have more.

Atomic Mass. Isotopes Reminder Yesterday we learned that the mass of all atoms of a certain element are not always the same –Some atoms may have more.
Isotopes and Weighted Averages

Isotopes and Weighted Averages
Isotopes Atoms of the same element that different mass numbers

Isotopes Atoms of the same element that different mass numbers
Average Atomic Mass The weighted average of the masses of all the naturally occurring isotopes of an element.

Average Atomic Mass The weighted average of the masses of all the naturally occurring isotopes of an element.
Average Atomic Mass.

Average Atomic Mass.
Isotopes  Atoms with the same number of protons but different numbers of neutrons  Ex) Carbon 12 vs. Carbon 14  These atoms have a different mass 

Isotopes  Atoms with the same number of protons but different numbers of neutrons  Ex) Carbon 12 vs. Carbon 14  These atoms have a different mass 
 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.

 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.
4.7 Atomic Mass Even the largest atoms have very small masses (Fluorine – 3.155 x 10 -23 ) Even the largest atoms have very small masses (Fluorine – 3.155.

4.7 Atomic Mass Even the largest atoms have very small masses (Fluorine – x ) Even the largest atoms have very small masses (Fluorine –
Using Isotope Data to Find a Weighted Average.  Each isotope will have two values associated with it.  Mass of Isotope  Percent Abundance (% found.

Using Isotope Data to Find a Weighted Average.  Each isotope will have two values associated with it.  Mass of Isotope  Percent Abundance (% found.

Similar presentations

Ads by Google