J OURNAL #21 Determine the # protons, neutrons and electrons for the following elements: Lithium Carbon-14 Iron (Fe)

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Presentation transcript:

J OURNAL #21 Determine the # protons, neutrons and electrons for the following elements: Lithium Carbon-14 Iron (Fe)

L EARNING G OALS We will write the hyphen notation for a given element. We will calculate the average atomic mass for a given element.

C OUNTING A TOMS Atoms of the same element have the same number of protons The atomic number of an element is the number of protons of each atom of that element Let’s practice Li B Cu Mg F

C OUNTING A TOMS Isotopes- atoms of the same element that have different masses The isotopes of a particular element have the same number of protons and electrons but different numbers of neutrons. Most of the elements consist of mixtures of isotopes Example: Hydrogen has 3 isotopes: protium, deuterium, tritium (radioactive Example: Tin has 10 stable isotopes (the most of any element)

M ASS N UMBER The mass number is the total number of protons and neutrons that make up the nucleus of an isotope. Examples: Carbon 12, 14, 16 Hydrogen 1, 2, 3 Isotopes are usually identified by specifying their mass number (exception hydrogen) Method known as Hyphen Notation Examples: Uranium 235 is written as: 235Mass # – atomic # = # of neutrons 235 (P+N) – 92 (protons) = 143 (neutrons) 92 U

H YPHEN N OTATION

P RACTICE : Write the hyphen-notation for the following isotopes: Carbon- 14 Helium- 4 Hydrogen- 3 Bromine- 80 Carbon- 13

R ELATIVE A TOMIC M ASS Masses of atoms expressed in grams are very small. Example: Oxygen-16 has a mass of x It is more convenient to use relative atomic mass The standard used to compare units of atomic mass is the carbon- 12 atom. It has been arbitrarily assigned a mass of exactly 12 atomic mass units or 12 amu One atomic mass unit (amu) is exactly 1/12 the mass of a carbon 12 atom

R ELATIVE A TOMIC M ASS Examples: Oxygen 16 has a mass of amu Magnesium 24 has the atomic mass of amu. Additional examples of atomic masses of the naturally occurring isotopes are on pg 82 in your textbook

A VERAGE A TOMIC M ASS Most elements occur naturally as mixtures of isotopes. The percentage of each isotope in the naturally occurring element on Earth is nearly always the same, no matter where the element is found. The percentage at which each of the element’s isotopes occurs in nature is taken into account when calculating the element’s average atomic mass Average atomic mass is the weighted average of the atomic mass of the naturally occurring isotopes of an element.

A VERAGE A TOMIC M ASS Example: Suppose you had a box containing 2 different size marbles. If 25% of your marbles have masses of 2.00g each and 75% have masses of 3.00g each, how is the weighted average calculated? You would count the number of each type of marble Calculate the total mass of the mixture Divide by the total number of marbles 25 marbles x 2.00g = 50g 75 marbles x 3.00g = 225g 50g + 225g = 275g Divide the total mass by 100 gives us the average marble mass of 2.75g

A VERAGE A TOMIC M ASS Example: Suppose you had a box containing 2 different size marbles. If 25% of your marbles have masses of 2.00g each and 75% have masses of 3.00g each, how is the weighted average calculated? A simpler method is to multiply the mass of each marble by the decimal fraction representing its percentage in the mixture: 25% = % = 0.75 (2.00g x 0.25) + (3.00g x 0.75) = 2.75g

A VERAGE A TOMIC M ASS The average atomic mass depend on both the mass and the relative abundance of each of the element’s isotopes. Examples: IsotopeMass #% Natural Abundance Atomic Mass (amu) Average Atomic mass Carbon-12 Carbon Oxygen-16 Oxygen-17 Oxygen Copper-63 Copper

A VERAGE A TOMIC M ASS Example: Suppose you had a box containing 2 different size marbles. If 25% of your marbles have masses of 2.00g each and 75% have masses of 3.00g each, how is the weighted average calculated? A simpler method is to multiply the mass of each marble by the decimal fraction representing its percentage in the mixture: 25% = % = 0.75 (2.00g x 0.25) + (3.00g x 0.75) = 2.75g