Download Chapter 3 Atoms and Elements Classification of Matter Matter Matter

Chapter 3 Atoms and Elements Classification of Matter Matter Matter is the “stuff” that makes up all things. Pure Substances A pure substance is classified as •
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matter with a specific composition. an element when composed of one type of atom. a compound when composed of two or more elements combined in a definite ratio. Elements are •
pure substances that contains atoms of only one type. Copper, Cu Lead, Pb Aluminum, Al Compounds •
contain two or more elements in a definite ratio. Salt (NaCl) Table sugar (C12H22O11) Water (H2O) Elements in a Compound “Table salt” is a compound that contains the elements sodium and chlorine. A mixture is a type of matter that consists of •
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two or more substances that are physically mixed, not chemically combined. •
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the composition is uniform throughout. •
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the composition of substances is not uniform. •
pure substances that cannot be separated into simpler substances by ordinary laboratory processes. •
the building blocks of matter. two or more substances in different proportions. substances that can be separated by physical methods. Physical Separation of A Mixture Example: Pasta and water are separated with a strainer. In a homogeneous mixture, the different parts of the mixture are not visible. In a heterogeneous mixture, the composition varies from one part of the mixture to another. the different parts of the mixture are visible. Classification of Matter Elements are Sources of Some Element Names Some elements are named for planets, mythological figures, minerals, colors, scientists, and places A symbol •
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represents the name of an element. •
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are observed or measured without changing its identity. •
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elements are arranged according to similar properties. •
use the letter A for the representative elements (1A to 8A) and the letter B for the transition elements. consists of 1 or 2 letters. starts with a capital letter. 1‐Letter Symbols 2‐Letter Symbols C carbon Co cobalt N nitrogen Ca calcium F fluorine Al aluminum O oxygen Mg magnesium Symbols from Latin Names Several symbols are derived from Latin names as shown below. Cu, copper (cuprum) Au, gold (aurum) Fe, iron (ferrum) Ag, silver (argentum) The physical properties of an element include the following: Shape Density Color Melting point Odor and taste Boiling Point Some physical properties of copper are: Color Red‐orange Luster Very shiny Melting point 1083°C Boiling point 2567°C Conduction of electricity Excellent Conduction of heat Excellent On the periodic table, groups contain elements with similar properties in vertical columns. periods are horizontal rows of elements. Group Numbers •
also use numbers 1‐18 to the columns from left to right. Names of Some Representative Elements Several groups of representative elements are known by common names. Alkali Metals Group 1A(1), the alkali metals, includes lithium, sodium, and potassium. Halogens Group 7A(17) the halogens, includes chlorine, bromine, and iodine. Metals, Nonmetals, and Metalloids The heavy zigzag line separates metals and nonmetals. •
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Metals are located to the left. Nonmetals are located to the right. Metalloids are located along the heavy zigzag line between the metals and nonmetals. Properties of Metals, Nonmetals, and Metalloids Metals •
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are shiny and ductile. •
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are dull, brittle, and poor conductors. •
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are better conductors than nonmetals, but not as good as metals. are good conductors of heat and electricity. Nonmetals are good insulators. Metalloids are used as semiconductors and insulators. In Dalton’s Atomic Theory, atoms •
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are tiny particles of matter. •
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protons have a positive (+) charge. •
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were aimed at atoms of gold. of an element are similar and different from other elements. of two or more different elements combine to form compounds. are rearranged to form new combinations in a chemical reaction. Subatomic Particles Atoms contains subatomic particles, electrons have a negative (‐) charge. like charges repel and unlike charges attract. neutrons are neutral. Rutherford’s Gold‐Foil Experiment In Rutherford’s gold‐foil experiment, positively charged particles mostly went straight through the atoms. were deflected only occasionally. Conclusion: There must be a small, dense, positively charged nucleus in the atom that deflects positive particles that come close. Structure of the Atom An atom consists •
of a nucleus that contains protons and neutrons. •
of electrons in a large empty space around the nucleus. Atomic Mass Scale On the atomic mass scale for subatomic particles, •
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1 atomic mass unit (amu) has a mass equal to 1/12 of the mass of the carbon‐12 atom. •
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is specific for each element. •
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Hydrogen has atomic number 1; every H atom has one proton. •
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an element is electrically neutral; the net charge of an atom is zero. •
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represents the number of particles in the nucleus. •
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are atoms of the same element that have different mass numbers. •
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represents a particular atom of an element. a proton has a mass of about 1 (1.007) amu. a neutron has a mass of about 1 (1.008) amu. an electron has a very small mass, 0.000549 amu. The atomic number is the same for all atoms of an element. is equal to the number of protons in an atom. appears above the symbol of an element. Atomic Number and Protons Examples of atomic number and number of protons: Carbon has atomic number 6; every C atom has six protons. Copper has atomic number 29; every Cu atom has 29 protons. Gold has atomic number 79; every Au atom has 79 protons. Electrons in An Atom has an equal number of protons and electrons. number of protons = number of electrons Aluminum has 13 protons and 13 electrons. The net charge is zero. 13 protons (13+) + 13 electrons (13 ‐) = 0 Mass Number The mass number is equal to the number of protons + the number of neutrons. Isotopes have the same number of protons, but different numbers of neutrons. A nuclear symbol gives the mass number in the upper left corner and the atomic number in the lower left corner. Example: An atom of sodium with atomic number 11 and a mass number 23 has the following atomic symbol: mass number 23 Na atomic number 11 Information from Nuclear Symbols From the nuclear symbol, we can determine the number of protons (p+), neutrons, (n), and electrons (e‐) in a particular atom. 16 31 65 O P Zn 8 15 30 8 p+ 15 p+ 30 p+ 8 n 16 n 35 n ‐
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8 e 15 e 30 e‐ Isotopes of Magnesium In naturally occurring magnesium, there are three isotopes. Isotopes of Sulfur A sample of naturally occurring sulfur contains several isotopes with the following abundances Isotope % abundance 32S 95.02 33S 0.75 34S 4.21 36S 0.02 Atomic Mass The atomic mass of an element •
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is listed below the symbol of each element on the periodic table. gives the mass of an “average” atom of each element compared to 12C. •
is not the same as the mass number. Isotopes of Some Elements and Their Atomic Mass Atomic Mass for Cl The atomic mass of chlorine is •
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due to all the Cl isotopes. •
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are assigned numbers n = 1, 2, 3, 4 and so on. not a whole number. the average of two isotopes: 35Cl and 37Cl. Energy levels increase in energy as the value of n increases. are like the rungs of a ladder with the lower energy levels nearer the ground. Energy levels have a maximum number of electrons equal to 2n2. Energy level Maximum number of electrons n = 1 2(1)2 = 2(1) = 2 n = 2 2(2)2 = 2(4) = 8 n = 3 2(3)2 = 2(9) = 18 Orbitals An orbital •
is a three‐dimensional space around a nucleus where an electron is most likely to be found. •
has a shape that represents electron density (not a path the electron follows). Electrons in Energy Levels Energy Total Level Electrons 1 2 2 8 ______________________ 3 18 4 32 Valence Electrons The valence electrons •
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determine the chemical properties of the elements. are the electrons in the highest energy level. are related to the group number of the element. Example: Phosphorus has 5 valence electrons. 5 valence electrons P Group 5A(15) 2, 8, 5 Groups and Valence Electrons All the elements in a group have the same number of valence electrons. Example: Elements in group 2A(2) have two (2) valence electrons. Be 2, 2 Mg 2, 8, 2 Ca 2, 8, 8, 2 Sr 2, 8, 18, 8, 2 Periodic Table and Valence Electrons Representative Elements Group Numbers 1 2 3 4 5 6 7 8 H He 2 1
Li Be Al C N O F Ne 2,1 2,2 2,3 2,4 2,5 2,6 2,7 2,8 Li Mg Ge Si P S Cl Ar 2,8,1 2,8,2 2,8,3 2,8,4 2,8,5 2,8,6 2,8,7 2,8,8 An electron‐dot symbol •
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shows the valence electrons around the symbol of the element. for Mg has two valence electrons as single dots on the sides of the symbol Mg. Writing Electron‐Dot Symbols Electron‐dot symbols for •
groups 1A(1) to 4A(14) use single dots. ∙ ∙ Na ∙ ∙ Mg ∙ ∙ Al ∙ ∙ C ∙ ∙ •
groups 5A(15) to 7A(17) use pairs and single dots. ∙ ∙ ∙ ∙ ∙ P ∙ : O ∙ ∙ ∙ Groups and Electron‐Dot Symbols In a group, all the electron‐dot symbols have the same number of valence electrons (dots). Example: Atoms of elements in Group 2A(2) each have 2 valence electrons. ∙ Be ∙ ∙ Mg ∙ ∙ Ca ∙ ∙ Sr ∙ ∙ Ba ∙ Atomic Radius Within A Group Atomic radius increases going down each group of representative elements. Atomic Radius Across a Period Going across a period left to right, •
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an increase in number of protons increases attraction for valence electrons. •
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the distance decreases between nucleus and valence electrons. •
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Metals have lower ionization energies. atomic radius decreases. Ionization energy is the energy it takes to remove a valence electron. Na(g) + Energy (ionization) Æ Na+(g) + e‐ Ionization Energy In a Group Going up a group of representative elements, the ionization energy increases. Ionization Energy Nonmetals have higher ionization energies.