Calculating the Average Atomic Mass. Steps for Calculating Average Atomic Mass (When given percentages of each isotope and each isotopes mass) 1. Convert.

Slides:

Advertisements

Similar presentations

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

Advertisements

Calculating Average Atomic Mass. Introduction The value for atomic mass for a particular element is the average atomic mass. Each sample of an element.

Average Atomic Mass Practice

Atomic Mass Standard mass unit is derived from carbon 12 Atomic mass unit – the mass equal to 1/12 the mass of one Carbon 12 atom.

AIM: HOW TO CALCULATE THE AVERAGE ATOMIC MASS? DO NOW:1. WHAT ARE THE 3 SUBATOMIC PARTICLES OF AN ATOM? LIST THE THREE SUBATOMIC PARTICLES AND THEIR CHARGE.

Chapter 11B Notes Determining Isotope Masses. Intro What is the mass of an atom with 6 protons and 6 neutrons? 12 What is the mass of an atom with 6 protons.

What is average atomic mass?

Average Atomic Mass.  An element can exist in a number of forms, called isotopes. Isotopes are forms of the same atom that vary in mass as a result of.

Average Atomic Mass.

Average Atomic Mass Due Monday Oct 14, 2013

 Definition: Atoms of the same element that differ in their # of neutrons; therefore, they have different mass numbers.  Nearly every element has isotopes!

Components of the Atom Nucleus: Nuclear Forces:

 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.

Examples: Average Atomic Mass. Example Chlorine exists as a mixture of % chlorine-35 and % chlorine-37. Determine the average atomic mass.

Isotopes and Mass Number. Atomic Number The number of protons in each atom identifies it as an atom of a particular element Each atom has a unique number.

Dalton was proved incorrect and his theory was modified

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.

Mass Number Atomic Number equals the # of... NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE ATOM.

Isotopes Atoms of the same element that different mass numbers

Number of Protons = Number of Electrons Number of Protons = Atomic Number Atomic Mass = Protons + Neutrons.

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

Average Atomic 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.

1 Atomic Mass The atomic mass of an element is listed below the symbol of each element on the periodic table. gives the mass of an “average” atom of each.

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

…AND THE AVERAGE ATOMIC MASS Isotopes. PG 88 GENERAL- ATOMS OF THE SAME ELEMENT BUT HAVE DIFFERENT AMOUNTS OF NEUTRONS IN THE NUCLEUS PAGE 54 PRE AP ATOMS.

 The weighted average of its naturally occurring isotopes. Chemical Name Atomic # Chemical Symbol Atomic Mass (Average Atomic Mass)

Average atomic Mass. What does the atomic mass tell us on the Periodic table?

Chapter 3 Average Atomic Mass. Section 3 Counting Atoms Relative Atomic Masses The standard used by scientists to compare units of atomic mass is the.

Average Atomic Mass How to use relative abundance to calculate average atomic mass.

Average Atomic Mass. Relative Atomic Masses  Masses of atoms (in grams) are very small, so for convenience we use relative masses.  Carbon-12 is our.

Determining Average Atomic Mass

What is average atomic mass?

Average Atomic Mass.   atomic masses reported in periodic table represent: weighted average of masses of all naturally occurring isotopes of an element.

Average Atomic Mass What is average atomic mass? Average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of.

Atomic Masses Test Friday!. Atomic Mass is an average (decimal) An average of known isotopes for an element The atomic mass of an element is closest to.

Average Mass Activity Find the average mass of all the spheres in the tray. You may: -Make no more than 3 mass measurements. -Mass only 1 sphere at a time.

Chapter 4 AVERAGE ATOMIC MASS. Atomic Mass… n The weighted average of the masses of all the naturally occurring isotopes of that element. n Is not a whole.

Isotopic Abundance Pages Thinking question Why are there decimal places for atomic masses on the periodic table if protons and neutrons have amu.

WEIGHTED AVERAGE MASS NUMBER: 1)The mass number on the periodic table is calculated from the weighted average of the most abundant isotopes. 2) Abundance.

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.

Comparing Atomic Mass and Mass Numbers Atomic Mass Mass Number The mass number is the total amount of protons and neutrons in an atom. An atom of an element.

This is the solution for carbon: (12) (0.9890) + (13) (0.0110) = amu mass number percent abundance % % Recall!!! carbon:

Average Atomic Mass!!!. Copper is made of two isotopes. Copper- 63 is 69.17% abundant and it has a mass of amu. Copper-65 is 30.83% abundant and.

Atomic Mass Mrs. Cook. Atomic Mass - The average relative mass of all naturally occurring isotopes of an element. relative mass – The mass of one object.

Average Atomic Mass Practice

Same Element Different Atom- Isotopes All atoms of a particular element are not exactly alike. Some elements have atoms with different masses (isotopes)

Isotopes are atoms of the same element that have a different number of neutrons For example, Hydrogen has 3 isotopes: Protium (0 neutrons) Deuterium (1.

Warm-Up -Write the correct Nuclide Symbol for the following elements: *19 p+, 20 n *82 e-, 125n *Mass # 238, neutrons= 146.

ATOMIC STRUCTURE THE NUCLEUS: 1) THE PROTON:

Calculating Atomic Mass

Calculating Average Atomic Mass

What is average atomic mass?

What is average atomic mass?

Average atomic Mass.

Estimating the Mass Number:

Average Atomic Mass.

ATOMIC STRUCTURE THE NUCLEUS: 1) THE PROTON:

A B 21085At Fe Mo 5827Co 3216S Pb4+ Symbol

Tuesday, September 23, 2014 Objective: Students will calculate the average atomic mass of common isotopes of an element. Warm-Up What do the following.

Isotopes and Average Atomic Mass

Atomic Structure.

Average Atomic Mass.

Average Atomic Mass.

Section 2.4 Atomic Weights.

Calculating Average Atomic Mass

Average Atomic Mass.

Average Atomic Mass.

Aim: How to Calculate the Average Atomic Mass?

Presentation transcript:

Calculating the Average Atomic Mass

Steps for Calculating Average Atomic Mass (When given percentages of each isotope and each isotopes mass) 1. Convert the percentages into decimals. (This percentage is known as its relative abundance or percent abundance). 2. Multiply the percentage of each isotope by its respective mass. 3. Add the numbers from step two together. Example: (percent abundance) (atomic mass) + (percent abundance) (atomic mass) (0.1883) (10.02 amu) + (0.8117) (11.01 amu) = amu IsotopeAtomic Mass (u)Natural Abundance % B amu18.83 B amu81.17

Independent Practice 1. Magnesium has three isotopes, Mg-24 (78.99%), Mg-25 (10.00%) and, Mg-26 (11.01%). Calculate the average atomic mass of magnesium. 2. The new element Mustangium (Mu) was discovered in 1998 by Mr. Abronowitz. It has three isotopes: Mu-284 (34.60%), Mu-285 (21.20%), and Mu-288 (44.20%). What is its average atomic mass? 3. Tellurium has eight isotopes: Te-120 (0.09%), Te-122 (2.46%), Te- 123 (0.87%), Te-124 (4.61%), Te-125 (6.99%), Te-126 (18.71%), Te- 128 (31.79%), and Te-130 (34.48%). What is its average atomic mass? 4. Silicon has two isotopes, Si-29 and Si-28. Find their percentages in nature. 5. In has two isotopes, In-115 which occurs 95.6% in nature. What is the mass of the other isotope?