NRAN80323_INORGANICchemistry_FALL23.pptx

INORGANIC CHEMISTRY Gregory Collins, DNP, CRNA PHYSICAL SCIENCE IN NURSE ANESTHESIA NRAN 80323 1 INORGANIC CHEMISTRY OBJECTIVES: READING: MEASUREMENT Nagelhout / Chapter 15 / MATTER 201-203 STATES CHANGES DALTON’S ATOMIC THEORY ATOMS AND MOLECULES CHEMICAL FORMULAS PERIODIC TABLE 2 WHAT IS CHEM...

INORGANIC CHEMISTRY Gregory Collins, DNP, CRNA PHYSICAL SCIENCE IN NURSE ANESTHESIA NRAN 80323 1 INORGANIC CHEMISTRY OBJECTIVES: READING: MEASUREMENT Nagelhout / Chapter 15 / MATTER 201-203 STATES CHANGES DALTON’S ATOMIC THEORY ATOMS AND MOLECULES CHEMICAL FORMULAS PERIODIC TABLE 2 WHAT IS CHEMISTRY? “…the STUDY OF MATTER and the CHANGES it undergoes.” “…the STUDY OF MATTER, COMPOSITION, PROPERTIES, and BEHAVIOR at the 3 MEASUREMENT Quantity SI Unit Mass Kilogram (kg) Length Meter (m) Volume Cubic meter (m3) Liter (L) Temperature Time Metric Unit Equivalents Gram (g) Meter (m) Kelvin (K) Second (s) 1 m = 3.280 ft m3=1000L = 264.2 gal Celsius (C) Second (s) 1 kg = 1000g = 2.205 lb Farenheit (F) Second (s) 4 MEASUREMENT 5 MATTER Anything that has MASS and takes up SPACE PROPERTIES OF MATTER PHYSICAL: • Characteristics • Behavior with environment CHEMICAL: • Ability to form new substance • 6 MATTER STATES (PHASES) OF MATTER GAS: • • • Has no definite shape or volume Expands to fill container Highly compressible LIQUID: • • No definite shape but definite volume Slightly compressible SOLID: • Definite shape and volume 7 MATTER COMPOSITION OF MATTER PURE SUBSTANCE vs MIXTURE ELEMENT vs COMPOUND 8 ELEMENT Simplest substance Cannot be broken down into smaller substances Combine to form COMPOUNDS One or two letter abbreviation for SYMBOL • first letter always capitalized • second letter, if present, always lower 9 ENERGY OF TRANSFORMATION PHYSICAL Changes • SPECIFIC HEAT (SH): Amount of heat necessary to raise temperature of 1.0 g of substance by 1.0° C • HEAT OF VAPORIZATION (DHovap): Amount of heat necessary to convert 1 mole of LIQUID to VAPOR at normal boiling point • HEAT OF FUSION (DHofus): Amount of heat necessary to convert 1 mole of SOLID to LIQUID at normal melting point CHEMICAL Changes • HEAT OF REACTION (DH): Heat released or absorbed in a chemical reaction  EXOTHERMIC reaction: RELEASES (gives off) heat  ENDOTHERMIC reaction: ABSORBS (takes on) heat 10 ENDOTHERMIC CHANGES SUBLIMATION • Direct conversion of a SOLID to a GAS (dry ice) MELTING or FUSION • Conversion of a SOLID to a LIQUID (melting ice) EVAPORATION or VAPORIZATION • Conversion of a LIQUID to a GAS 11 EXOTHERMIC CHANGES CONDESATION or LIQUIFICATION • Conversion of a GAS to a LIQUID or solid (steam to water) FREEZING or CRYSTALLIZATION • LIQUID becomes a SOLID (ice formation) (Substances usually first condense to liquids and then become solids) 12 DALTON’S ATOMIC THEORY John Dalton (1766-1844) DALTON’S ATOMIC THEORY (1808) • All matter composed of very tiny particles, called ATOMS • All atoms of same element have same chemical properties • Atoms of different elements have different chemical properties • COMPOUNDS formed by chemical combination of two or more different kinds of atoms • A MOLECULE is a tightly bound combination 13 ATOMS Smallest, most basic particle of an ELEMENT Composed of three subatomic components: PROTONS: • POSITIVELY CHARGED particles in the NUCLEUS • Carry an equal, opposite charge to electrons, but much larger and heavier ELECTRONS: • Surround the nucleus, and are only found in ORBITALS • Orbitals have fixed energy values called quantum • Diffuse region of NEGATIVE CHARGE NEUTRONS: 14 SUBATOMIC PARTICLES 15 ATOMS ATOMIC NUMBER (Z): Number of protons in nucleus of atom • • • • Atoms of same element have same number protons Atoms of different elements have different number protons Represented by WHOLE-NUMBER on periodic table In a neutral atom, number protons equal to number electrons ISOTOPES: Atoms with same number of protons but different number of neutrons • MOST elements found on Earth are mixtures of isotopes 16 ATOMS MASS NUMBER (A): SUM of the NUMBER of PROTONS and NEUTRONS in nucleus of an atom • Electrons are NOT counted in determining mass number • NOT found on periodic table ATOMIC MASS (ma): Weighted AVERAGE MASS of an atom of an element based on the natural relative abundance of that element’s isotopes • Also known as ATOMIC WEIGHT • Represented by DECIMAL-NUMBER on periodic table 17 ATOMS 18 MOLE • The amount of a substance whose MASS in grams is numerically EQUAL to its MOLECULAR or formula WEIGHT • The average ATOMIC MASS of an element, when expressed in grams, is 1 mol of that kind of atom • The molecular weight of a molecule is the average mass (based on ATOMIC MASS) of a substance’s molecules • Atoms, ions, and molecules which are too small to measure in grams can be related by using the AMU or Atomic Mass Unit • AVAGADRO’S NUMBER: 6.022 x 1023...allows for calculation of NUMBER of ATOMS or MOLECULES in 1 mol 19 MOLE • Enables chemists to essentially COUNT atoms by MASSING them • Provides a practical, working UNIT when considering chemicals • Think in terms of a “dozen” or “six-pack” 20 CHEMICAL FORMULAS Chemical SYMBOLS of elements in the chemical formula represent the ELEMENTS present (perchloric acid HClO4) Subscript numbers represent mole proportions of the proceeding elements, no subscript number implies a subscript of 1 (perchloric acid HClO4 = 1 H, 1 Cl, 4 O) Formula can be expressed as EMPERICAL, MOLECULAR, or STRUCTURAL EMPERICAL formula: C2H4O2 acetic acid Only shows types and numbers of atoms present in molecule, least informative MOLECULAR formula: CH3COOH acetic acid 21 PERIODIC TABLE OF ELEMENTS Dmitri Mendeleev (1834-1907) Arranged known elements in order of increasing atomic weight. He observed certain sets of properties recur periodically. He arranged elements with similar properties in same column or GROUP/FAMILY. Horizontal rows are22 PERIODIC TABLE OF ELEMENTS 23 PERIODIC TABLE OF ELEMENTS 24 PERIODIC TABLE OF ELEMENTS 25 PERIODIC TABLE OF ELEMENTS • PROPERTIES of the elements vary in a PERIODIC manner • Helps to understand the behavior, reactions, and properties of the elements • Moving from left to right in a PERIOD of the periodic table, the properties of the elements gradually change • At the end of each row, a drastic shift occurs in chemical properties • The next element in order of atomic number is more similar to the first element in the row 26 27 PERIODIC TABLE OF ELEMENTS BOHR MODEL: electrons are not located randomly around nucleus of atom, but rather occur in specific electron shells PERIODIC nature of chemical properties is related to the ELECTRON CONFIGURATION of the atoms of the elements • Each shell has a limited capacity for electrons • As lower shells are filled, additional electrons reside in more distant shells • The electrons of an atom occupy quantum levels or orbitals starting from the lowest energy level, and proceeding to the highest • Each orbital has a maximum of two paired electrons (opposite spins) 28 PERIODIC TABLE OF OCTET RULE OF ELECTRON FILLING ELEMENTS • Atoms are most stable if they have filled or empty outer layer electrons • Except for H and He, a filled layer contains 8 electrons or an OCTET • Atoms gain, lose, or share electrons to make a filled or empty outer layer • Atoms gain, lose, or share electrons based on what is easiest, gaining or loosing 29 PERIODIC TABLE OF ELEMENTS 30 PERIODIC TABLE OF ELEMENTS 31 PERIODIC TABLE OF ELEMENTS 32 PERIODIC TABLE OF ELEMENTS METALS: ductile & malleable, shiny; most are solids • GOOD CONDUCTORS of electricity • Form alloys • Tend to GIVE UP ELECTRONS in chemical reactions NONMETALS: solids tend to be dull & brittle, many are gases • POOR CONDUCTORS of electricity • Tend to ACCEPT ELECTRONS reacting with metals, SHARE when reacting with other nonmetals • Many exist as diatomic molecules (Cl2, Br2, I2) 33 PERIODIC TABLE OF ELEMENTS 34 PERIODIC TABLE OF ELEMENTS ALKALINE METALS: • Only one electron in outer valence shell • Easily give up electron, very reactive • Commonly exist as cations (Na+, K+) ALKALINE EARTH METALS: • Two electrons in outer valence shell • Relatively reactive • Can exist as cation with 2+ NOBLE GASES: • Inert, do not react • FULL outer valence shell HALOGENS: • One electron short of valence octet • Easily take on single electron to fill outer valence • Among the most reactive of the elements 35 SUMMARY UNDERSTANDING: What are the routine units of measure in chemistry? Define and describe the properties, phases, and composition of matter. What is an element? Describe the types of energy involved in physical and chemical change. List and differentiate endothermic and exothermic changes. Summarize Dalton’s Atomic Theory. Define atoms in terms of subatomic components. What is a mole and why is it useful? Understand the components of chemical formulas. Describe the arrangement of the periodic table in terms of chemical properties. Understand how chemical and physical properties change by moving along a period and between a group. What is the octet rule of electron filling? Define and differentiate metal, nonmetals, and metalloids. List the distinct properties of alkaline metals, earth metals, halogens, and noble gases. 36