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PHYSICAL-SCIENCE-2019.pptx
- 1. GEN-ED PHYSICAL SCIENCE RUTHER FRANCISTABLATE, LPT
- 2. Physics, Chemistry &Biology
- 12. SCIENTISTS • PTOLEMY (EarthCentered Model - geocentric) • GALILEO (Telescope) • COPERNICUS (Sun Centered Model – heliocentric) • JOHANNES KEPLER (Laws of Planetary Motion) • TYCHO BRAHE (Detailed observation of heavenly bodies without aid of telescope)
- 13. KEPLER’S LAWS 1. Lawof Ellipses Orbit of the planets is eccentric Orbit can be highly elleptical (round) Orbit can be non-highly elleptical (flat)
- 14. KEPLER’S LAWS 2. Lawof Equal Areas A radius vector joining any planet to the sun sweeps out equal areas in equal time
- 15. KEPLER’S LAWS 3. Lawof Period The shorter the revolution of a planet around the sun, the shorter it’s orbit
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- 34. PERIODIC TABLE OFELEMENTS
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- 37. MATTER Occupies Space Has Mass Has Weight Has Properties Extensive Mass x Acceleration due toGravity (g) Earth - 9.8 m/ Moon – 1.6 m/ Sun - 270 m/ Intensive -Mass -Size -Volume -Length -Width -Height -Density -Boiling point -Freezing point -Melting point
- 38. PHYSICAL PROPERTIES OFMATTER
- 39. INTENSIVE PROPERTIES OFWATER • Density = M / V = 1.000g/ml • Boiling point = 100 degC • Freezing point= 0 degC
- 40. Substance Not pure Pure Element Compound -Metal -Non-Metal -Metalloids OrganicInorganic With Carbon -CO4 -NaHCO3 Without Carbon -Salts -Acids (H+) -Base (OH) -Water
- 42. CHANGES • Physical -affects form but not chemical composition
- 43. CHANGES • Chemical -one or more new substances are formed
- 44. Factors Affecting Changes •Amount of Substance - (mol, particles) • Time - (s, min, hr) • Temperature - (C, F, K) • Mass - (g, kg, lbs) • Length - (m, in, ft) • Distance / Displacement - (m, in, ft) • Electric Current - (amp) • Luminous intensity - (cd) • Pressure - (P, bar, atm, torr)
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- 47. SCIENTISTS • Amadeo Avogadro •Anton Lavoisier • Joseph Prousz • Niels Bohr (Planetary Model of Atom) • Henry Moseley (atomic number justification) • Goldstein & Rutherford (protons) • JJ Thompson (electron) • James Chadwick (neutron)
- 48. Amadeo Avogadro • Fundamentalunit of matter • Avogadro’s Number NA = 6.022 x 10 - numbers of elementary particles - proportion - atomic scale vs human scale
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- 52. Metal + Non Metal NonMetal+ Non Metal
- 53. Formulas for writingSubstances • Molecular - shows actual number of atoms • Empirical - shows the ratio of atoms 6:12:6 = 1:2:1
- 54. X = Element A=Atomic Mass Z = Atomic Number n = neutron p+ = protons e- = electrons A = p+ + n n = A - z Determining numbers of particles using Atomic Mass and Atomic Number
- 55. ELECTRONIC CONFIGURATION • Inatomic physics and quantum chemistry, the electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbitals. For example, the electron configuration of the neon atom is 1s2 2s2 2p6.
- 56. Energy Levels •7 Energy Levelsor Shells •Numbered 1- 7 or K-Q
- 57. In showing ElectronicConfiguration • Elements • Atomic Number of element • Electrons (core, outer / valence) • Energy levels • Orbitals • Pauli’s exclusion principle • Hund’s Rule of electron pairing • Afbau Building Principle • Octet rule
- 59. Examples of ChemicalBonding
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- 65. • Metals absorbsheat better than non metals C = (F-32)(5/9) F = (C)(9/5)+32 K = C +273.15 HEAT
- 66. ENERGY • Potential Energy- At rest • Kinetic Energy - In motion
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- 68. Work • For workto be done, there has to be movement or displacement done over a period of time W = Fd
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