Chemistry B11 Chapter 3 Atoms.

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Presentation transcript:

Chemistry B11 Chapter 3 Atoms

Matter Pure substances Mixtures Element Compounds Homogeneous matter Anything that occupies space and has mass Pure substances Fixed composition, cannot be more purified Mixtures A combination of two or more pure substances Physically Separable into Element Cannot be subdivided by chemical or physical means Compounds Elements united In fixed ratios Homogeneous matter Uniform Composition throughout Heterogeneous Nonuniform composition Combine Chemically To form

Element: Is a substance consisting of “identical” atoms. Cannot be separated by chemical or physical methods. Carbon, Hydrogen, Oxygen 116 elements – 88 in nature Compound: A pure substance made up of two or more elements in a fixed ratio by numbers. H2O (Water): 2 Hydrogen & 1 Oxygen CO2: 1 Carbon & 2 Oxygen 20 million compounds

H2O CO Compounds Formula Identifies each element Ratios H O 2 = 1 or 2 : 1 C 1 : 1 H2O CO

H2O CH4 Molecular models O H H C Molecular formula Structural Ball-and-stick model Space-filling C H CH4

Mixtures Mixture: is a combination of two or more pure substances. Homogeneous: uniform throughout Air, Salt in water Heterogeneous: nonuniform Soup, Milk, Blood

Law of conservation of mass: C + O  CO All matter is made up of very tiny, “indivisible” particles (atoms). All atoms of a given element have the same chemical properties. Compounds are formed by the chemical combination of two or more different kinds of atoms. 4. A molecule is a bound combination of two or more atoms. Dalton’s Atomic theory

Monatomic Ar He Diatomic N2 O2 Polyatomic Element: S8 Atom

Atom Nucleus: positive charge Atoms are neutral.                                                                                        Atoms are neutral.                                                                                        Atomic mass unit (amu) = 1.6605×10-24 g mass of proton = 1 amu mass of neutron = 1 amu mass of electron = 5.48×10-4 amu

C Atom Mass number (A): Protons + Neutrons Atomic number (Z): Protons 12 6 Mass number Atomic number

Isotopes Isotopes: atoms with the same number of protons and electrons but different numbers of neutrons. different mass numbers C 12 6 C 13 6 C 14 6 6 P + 6 N 6 P + 7 N 6 P + 8 N Almost the same properties

Cl Cl Atomic Weight Cl Cl Atomic weight: of an element is average of the masses (in amu) of its isotopes found on the Earth. Cl 35 37 Cl Cl 34.97 amu 36.97 amu 17 17 (75.77/100 × 34.97 amu) + (24.23/100 × 36.97 amu) = 35.45 amu Cl 17 35.45 Atomic number Atomic weight

Main-group elements: 1A to 8A Transition elements: 1B to 8B (3 – 12) Inner transition elements: between B3 & B4 (58 to 71 and 90 to 103) Column: same properties (main group) Row or Period

VERY reactive, unstable, solid metal Group 1A: Alkali metals Li-Na-K-Rb-Cs-Fr VERY reactive, unstable, solid metal 2Na + 2H2O 2NaOH + H2 2Na + Cl2 2NaCl Group 2A: Alkali Earth metals Be-Mg-Ca-Sr-Ba-Ra reactive, solid metal

reactive, colored, gas, nonmetal Group 7A: Halogens F-Cl-Br-I-At reactive, colored, gas, nonmetal Group 8A: Noble gases He-Ne-Ar-Kr-Xe-Rn non reactive, stable, gas, nonmetal

Classification of the elements metals nonmetals metalloids metals: solid (except mercury), shiny, conductors of electricity, ductile, malleable nonmetals: solid, liquid or gas, do not conduct electricity (except graphite) metalloids: between metals and nonmetals

Metallic properties More metallic More metallic

Maximum number of electrons Bohr model n=1 n=2 n=3 n=4 n=5 E1 E2 E3 E4 E5 Principal energy levels or Shells E1 = ground state: lowest energy level 32 4 18 3 8 2 1 Maximum number of electrons Shell Lower energy Higher energy

Subshell: s p d f Orbital: is a region of space and it can hold 2 electrons (max). s px py pz magnetic field paired spins

Subshell: s p d f s p d f 2 2+2+2=6 2+2+2+2+2=10 2+2+2+2+2+2+2=14

Maximum number of electrons Shell Orbitals Maximum number of electrons 1 1s 2 2s, 2p 2 + 6 = 8 3 3s, 3p, 3d 2 + 6 + 10 = 18 4 4s, 4p, 4d, 4f 2 + 6 + 10 +14 = 32 3 2 3d 3p 3s 2p 2s Principal energy level Orbitals Energy 1 1s

Electronic configuration: description of the orbitals that its electrons occupy. Orbital box diagrams Electron configuration H (1) 1s 1s1 1s He (2) 1s2 Li (3) 1s 2s 1s2 2s1 C (6) 1s 2s 1s2 2s2 2p2 2px 2py 2pz

Noble gas notation 1s2 2s1 Li (3) [He] 2s1 1s2 2s2 2p5 F (9) [He] 2s2 2p5 2px 2py 2pz Si (14) 1s 2s 3s 2px 2py 2pz 3px 3py 3pz 1s2 2s2 2p6 3s2 3p2 [Ne] 3s2 3p2

Valence shell: outer shell Valence electrons: outer-shell electrons Cl (17) 1s2 2s2 2p6 3s2 3p5 7 valence electrons Ar (18) 1s2 2s2 2p6 3s2 3p6 8 valence electrons C (6) 1s2 2s2 2p2 4 valence electrons 1s2 2s2 2p6 8 valence electrons Ne (10) Noble gases Filled valence shells

For Main-group elements: Elements in the same column (group) have the same number of electrons in their valance shells. The same chemical and physical properties And form the same number of bonds.

Lewis dot structure Cl H He Li C 1A 2A 3A 4A 5A 6A 7A 8A

Main groups elements s, p Transition elements s, p, d Inner transition elements s, p, d, f

Atomic Size Size of an atom: is the size of its outermost occupied orbital. d

Ionization Energy Li + energy → Li+ + e- ion Ionization energy: the energy required to remove the most loosely held electron from an atom in the gaseous state. Ionization energy Ionization energy