Elements and Atoms NEVER TRUST AN ATOM THEY MAKE UP EVERYTHING
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1 Elements and Atoms NEVER TRUST AN ATOM THEY MAKE UP EVERYTHING
2 Atoms Matter! All matter is made up of tiny, fundamental particles called atoms Atoms are the smallest particles of an element that retain the physical and chemical properties of that element So how small is an atom? Most atomic radii fall within a range of 50 to 200 pm 1 mm = 10 9 pm!!!!!
3 How do we know atoms exist? Democritus had an idea he believed that all matter was composed of indivisible and indestructible particles called atoms. Democritus (460 B.C 370 B.C) Unfortunately, his idea was limited because it could not explain chemical behavior and he lacked experimental support.
4 How do we know atoms exist? In the late 1700 s and early 1800 s, John Dalton studied the ratios in which elements combine in chemical reactions. He formulated hypothesis and theories to explain his observations. The result of his work was the formulation of Dalton s Atomic Theory.
5 All elements are composed of tiny indivisible particles called atoms. Atoms of the same element are identical. The atoms of any one element are different from those of any other element. Atoms of different elements can physically mix together or can chemically combine in simple wholenumber ratios to form compounds. Chemical reactions occur when atoms are separated, joined, or rearranged. Atoms of one element are never changed into atoms of another element in a chemical reaction.
6
7 Subatomic Particles We now know that all atoms are comprised of 3 subatomic particles: Protons are positively charged particles located in the nucleus of an atom. The mass of a proton is equal to that of a neutron. Neutrons are also located in the nucleus of an atom. However, they do not have a charge (neutral). The mass of a neutron is equal to that of a proton. Electrons are negatively charged particles that surround the nucleus of an atom. Bohr Diagram
8 Subatomic Particle: Summary Particle Symbol Relative Charge Relative Mass Mass (grams) Proton p x Neutron n x Electron e 1-1/ x 10-28
9 Elements: Why are they different? Elements are different because their atoms contain different numbers of protons All atoms of a given element have the same number of protons The atomic number of an element is the number of protons in the nucleus of an atom of that element In a neutral atom the number of protons is equal to the number of electrons Carbon 6 C Element Name Atomic Number Chemical Symbol Atomic Weight
10 Elements and the Periodic Table Using the Periodic Table, find the following elements: Hydrogen Helium Lithium Beryllium Boron Draw the element squares and label the following: element name, atomic number, chemical symbol, and atomic mass How many protons and electrons are in each neutral atom?
11 Mass Number The mass number is the sum of the number of protons and the number of neutrons in an atom mass number = p + + n 0 If the mass number of chlorine is 35, how many neutrons are in a chlorine atom? If the mass number of gold (Au) is 197, how many neutrons are there in the gold atom?
12 Mass Number: Shorthand Notation The mass number of an element is usually indicated using shorthand notation There are two ways to indicate the mass number: Gold Au
13 Isotopes All atoms of a given element have the same atomic number However, most elements consist of atoms having several different mass numbers What does this imply? Atoms of an element having different mass numbers are called isotopes Isotopes of an element have the same number of protons, but different number of neutrons
14 Isotopes
15 Mini-Quiz All atoms are comprised of 3 subatomic particles:,, and Positively charged particles are called and are located Negatively charged particles are called and are located Elements differ from one another because The atomic number of an element is An atom of a given element will always have the same number of, but could have a different number of
16 Atomic Structure: Bohr Model Diagrams There are two models that are commonly used to describe the structure of an atom: the Bohr model and the quantum mechanical model. The Bohr model is not completely accurate. However, it is often used to help beginning chemistry students visualize the structure of an atom. According to this model, electrons are found in discrete energy levels, or shells. + Each ring represents an energy level
17 Atomic Structure: Bohr Model Diagrams Each energy level can hold a maximum number of electrons: n = 1 n = 2 n = 3 n = 4 2 electrons 8 electrons 18 electrons 32 electrons + n = 1 n = 2 n = 3 n = 4 We always fill the shells from lowest energy to higher energy. The higher the value of n, the higher the energy. Each ring represents an energy level
18 Drawing Bohr Model Diagrams Draw a Bohr model diagram for carbon-12 and chlorine-35.
19 Preview: Quantum Mechanics Electrons of an atom are located in distinct energy levels (as indicated by the Bohr model). However, we now know that these electrons do not orbit the nucleus of an atom. If electrons are not revolving around the nucleus, then where are they? According to the QM model, we cannot know the exact location of an electron. However, we can describe the probability of finding an electron in a given region of space (3 dimensions). Orbitals define these regions of space.
20 Atomic Orbitals There are several different types of orbitals: s p d f
21 Atomic Orbitals
22 Energy Levels, Orbitals, and Electrons Energy Level (n = ) Orbitals Maximum # of electrons Electron configuration spdf notation
23 Atomic Mass You may have noticed that the mass number of an element is always very close to its atomic weight (there s a reason!) The atomic weight of element is expressed in atomic mass units (u) What exactly is an atomic mass unit? Scientists assigned carbon-12 an atomic mass of 12 u. One atomic mass unit, 1 u, is defined as 1/12 of the mass of a carbon-12 atom.
24 Atomic Mass The atomic weight of element is expressed in atomic mass units (u) What exactly is an atomic mass unit? The atomic mass unit is based on the carbon-12 atom. The atomic mass of carbon-12 is exactly 12 u. Since carbon-12 consists of 6 protons and 6 neutrons, each nuclear particle has a mass of 1 u.
25 Atomic Mass Particle Mass (grams) Mass (u) Proton x Neutron x Electron x Atomic mass units are convenient to use in calculations. However, we may need to convert to units of grams. To do so, we can use the following conversion factor: 1 u = x g
26 Atomic Weight The atomic weight of an element is the average mass of a representative sample atoms Neon-20 Neon-21 Neon u 21 u 22 u What do you think the average mass of Neon might be? Use the periodic table to check your prediction.
27 Atomic Weight & Isotopes Isotopes are not present in equal quantities. Therefore, we cannot use a standard average. We must consider the percent abundances of each isotope. percent abundance = number of atoms of a given isotope total number of atoms (all isotopes of the element) 100 Neon-20 Neon-21 Neon-22 Number of atoms: Calculate the percent abundance of each isotope.
28 Atomic Weight: A Weighted Average Calculating the atomic weight: Atomic weight = % abundance isotope A 100 mass isotope A + % abundance isotope B 100 mass isotope B Neon-20 Neon-21 Neon-22 Percent abundance: Atomic mass: Calculate the atomic weight of Neon. Use the periodic table to check your prediction.
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