1 amu 1 amu 0 amu. Chapter 2 part 1.notebook September 16, Modern Atomic Theory

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1 Chapter 2 The Atom Elements are the basic substances that make up all matter. An atom is the smallest particle of an element. Average atoms are m in diameter. If you could put 6.02 x p + and n o on a scale they would have a mass of about 1g. Therefore: Recall: Subatomic Particle Charge Symbol Mass Atomic Mass Unit 1 amu 1 amu 0 amu This makes it inconvenient to measure in grams so chemists use the ATOMIC MASS UNIT (u) Modern Atomic Theory 1.All matter is made of tiny particles called atoms. Each atom is made of subatomic particles: p +, n o and e 2.Atoms of one element cannot be converted into atoms of another element by chemical reactions. 3.Atoms of 1 element have the same properties. These are different than other elements 4.Atoms combine in specific proportions to form compounds. Recall: Standard Atomic Notation X = ATOMIC SYMBOL = A = ATOMIC MASS = Z = ATOMIC NUMBER= How do you infer the number of electrons?

2 ISOTOPES (Chapter 5.1) All neutral atoms of the same element contain the same numbe of PROTONS and ELECTRONS. The number of neutrons can vary. Example: In nature most O atoms have 8 neutrons and a mass of 16. However O can also have 9 or 10 neutrons. These 3 forms are called ISOTOPES. Ex u % u % isotopic abundance Isotopes have the same # of p + but a different # of n o All the isotopes have similar chemical properties, but some of them are more UNSTABLE than others. Unstable means that their nuclei are more likely to DECAY or come apart releasing energy and subatomic particles. This is called RADIOACTIVITY and the atoms are called RADIOISOTOPES.

3 Radiation types: ionizing radiation (gamma (γ) uv, x rays) beta (β) = fast moving e alpha (α) = fast moving e and 4 2He +2 n 0 p + e Isotopes of Hydrogen 1 1 H stable hydrogen H H deuterium (heavy hydrogen) H 2 little bit radioactive 3 1 H tritium H 3 radioactive p + p + p + n 0 n 0 n0 p + n0 ATOMIC MASS and ISOTOPES Refer to Chapter 5 for the following information water: H 2 O mass: 18amu heavy water: D 2 O mass: 20amu Atomic mass units are a RELATIVE measure related to the mass of carbon 12 1 atom of carbon has been assigned a mass of 12u. This is the same as saying 1u is equal to 1/12 the mass of one carbon atom. The mass of all other atoms are measured relative to carbon 12 Most elements are made up of 2 or more isotopes. = 2000 isotopes in nature (stable and radioisotopes)

4 Because isotopes have different #s of neutrons, they have different masses. This must be accounted for when determining the mass of 1 atom of an element. For example Mg has 3 naturally occurring isotopes. 24Mg, 25 Mg, and 26 Mg. These isotopes are present in different amounts. In nature 79% of Mg is found as 24 Mg, 10% as 25 Mg, and 11% as 26 Mg. The relative amount of each isotope is called the ISOTOPIC ABUNDANCE. To determine the mass of a Mg atom the isotopic abundance must be accounted for. AVERAGE ATOMIC MASS The AVERAGE ATOMIC MASS of an element is the average masses of all the isotopes of that element. The mass given for each element on the periodic table is the average atomic mass To determine the isotopic abundance and the mass of each isotope, chemists use a device called a MASS SPECTROMETER Once the data is obtained the average atomic mass can be calculated by finding the WEIGHTED AVERAGE Average Atomic Mass = (% 24 Mg)( 24 Mg Mass) + (% 25 Mg)( 25 Mg Mass) + (% 26 Mg)( 26 Mg Mass) = (.79)( u) + (.10)( u) + (.11)( u) =

5 You try chlorine: If you know the average atomic mass of an element and the masses of its isotopes you can calculate the isotopic abundance of each isotope amu Example: Boron exists as two naturally occurring isotopes: 10 B (10.01u) and 11B (11.01u). Boron has an average atomic mass of 10.81u. Calculate the isotopic abundance of each isotope. You try: Silver (Atomic weight ) has two naturally occurring isotopes with isotopic weights of and What is the percentage abundance of each isotope? Let x be the % abundance of B 10, then 1 x is the % B = x(10.01) + (1 x)(11.01) = 10.01x x = 10.01x 11.01x 0.2 = x %B 11 = 1 x 0.2 = x = = 0.8 There is 20.00% B 10 and 80.00% B 11

6 In a sample of 400 lithium atoms, it is found that 30 atoms are lithium 6 (6.015 amu) and 370 atoms are lithium 7 (7.016 amu). Calculate the average atomic mass of lithium. Gallium has an average atomic mass of amu. If it is made up of isotopes with masses of amu and amu, what is the percent abundance of each isotope? Electrons Electrons occupy space around the nucleus. The hit list questions from pg 167 & 170 should be completed in this chapter

7 They are the first subatomic particle to interact when atoms get close together. The # of e and their arrangement will determine how a particular atom reacts. Electrons are restricted to fixed regions (probability clouds) around the nucleus called orbitals. These are volumes of space where the e can be. You probably called these orbits (Bohr Rutherford) We are now going to call them ENERGY LEVELS. e close to the nucleus have LESS ENERGY so they are in a LOWER ENERGY LEVEL. Recall: There is a certain # of electrons that each energy level can hold. The energy levels in atoms and the arrangement of electrons is very closely related to the structure of the PERIODIC TABLE OF THE ELEMENTS. How is this book shelf the same?

8 The Periodic Table Dmitri Mendeleev ( ), sequenced the known elements (65) in order of increasing atomic mass. The result was a table of the elements, organized so that elements with similar properties were arranged in the same column. This organization resulting in periodic (repeating) of patterns and was called the PERIODIC TABLE OF THE ELEMENTS Mendeleev's 1869 periodic table 1871 version

9 mendeleev's table! The modern periodic table is arranged by atomic number and the PERIODIC LAW: The chemical and physical properties of the elements repeat in a regular, periodic pattern when they are arranged according to their atomic number The periodic trends (repeating patterns) that result from organizing the elements by their atomic number are linked to the way in which electrons occupy and fill energy levels. Remember Bohr Rutherford Diagrams? Try 1.

10 Remember Bohr Rutherford Diagrams? There are a couple of important patterns that emerge when you draw Bohr Rutherford diagrams of the elements. There is a more convenient way to represent atoms than B/R diagrams. Lewis diagrams (grade 10) use the atomic symbol and show only the valence electrons to represent an atom. 1.An element s period number is the same as the number of energy levels that the electrons of its atoms occupy. 2.The elements in Groups 1 (1A), 2 (2A), and 13 (3A) to 18 (8A). All the elements in each main group have the same number of electrons in their highest (outer) energy level. These are known as VALENCE ELECTRONS. Valence e are responsible for the chemical behaviour of elements. Stable Atoms Group 18 (VIII A) are the only elements that exist as individual atoms in nature. They are very UNREACTIVE. Since chemical reactivity is determined by valence electrons, there must be something about the noble gases electron arrangement that makes them so unreactive. All the noble gases have outer energy levels that are completely filled with the maximum number of electrons. What does this stability mean? It means that a full outer energy level is unlikely to change. Scientists have observed that, in nature, situations or systems of lower energy are favoured over situations or systems of higher energy. When atoms have eight electrons in the outer energy level, they have lower potential energy, and we say they have a STABLE OCTET.

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