Classification of Matter

1
(No Transcript)
2
(No Transcript)
3
(No Transcript)
4
(No Transcript)
5

• Classification of Matter
• Classification by Physical State
• A gas is a state of matter in which the matter
  has no fixed volume or shape.
• A liquid is a state of matter in which the matter
  has a fixed volume that takes on the shape of
  its container.
• A solid is the state of matter with both fixed
  volume and shape.
• Classification by Composition
• Pure Substances have a fixed composition and
  distinct properties.
• Elements
• Compounds made up of two or more elements.
• Mixtures are combinations of two substances that
  have a composition that can vary.
• Homogeneous mixtures, or solutions, have the same
  composition throughout their volume.
• Heterogeneous mixtures have a composition that
  varies throughout their volume.

6
(No Transcript)
7
(No Transcript)
8

• Properties of Matter
• Chemical properties of matter describe how one
  kind of matter interacts with another kind of
  matter.
• Examples butane burns in air, water does not
  burn in air
• Physical properties of matter are not dependent
  on how one kind of matter interacts with
  another kind of matter.
• Examples temperature, color, the state of matter
  at a temperature
• Extensive properties of matter depend on the
  amount of matter - the extent of the sample of
  matter - under investigation.
• Examples mass, volume
• Intensive properties are properties of intensity
  and do not depend on the amount of matter in
  the sample under investigation.
• Examples color, temperature, density, chemical
  properties

9

• Physical and Chemical Change
• Physical Change does not involve a change in the
  chemical identity of a substance even though it
  may have changed its physical state or gross
  size and shape
• Examples
• Heating a sample of matter to a higher
  temperature
• Melting a substance
• Evaporating a liquid
• Chemical Change involves converting one or more
  substances into other substances
• Examples
• Reacting hydrogen with oxygen 2H2(g) O2(g)
  2H2O(l)
• Combustion of methane with oxygen CH4(g)
  2O2(g) CO2(g) 2H2O(l)

10

• Units of Measure
• Le Système International dUnités - The SI Units
• 7 Base Units
• Length meter (m) - the distance light travels
  in 1/199,792,458 seconds.
• Mass kilogram (kg) - the mass of a standard
  block of Pt-Ir alloy in Paris.
• Time second (s) - the duration of 9,192,631,770
  oscillations of the light emitted from Cs
  atoms.
• Amount of Substance mole (mol) - the mass of
  sample containing the same number of
  fundamental particles as are in exactly 12 grams
  of
• Temperature kelvin (K) - a change in temperature
  of 1 K is the same as 1 ºC. 0 K is defined at
  the temperature of the triple point of water -
  the condition when gaseous, liquid and solid
  water are in equilibrium. This turns out to be
  0.01 ºC and 273.16 K. Therefore K ºC 273.15
  because the freezing point of water is 0 ºC or
  273.15 K.
• Electric current ampere (A)
• Luminous intensity candela (cd)

11

• Decimal Conversions
• Unit prefixes indicate a multiplier or divisor of
  the base unit
• kilo (k) 1,000 103
• mega (M) 1,000,000 106
• giga (G) 1,000,000,000 109
• _______________
• deci (d) 10-1
• centi (c) 10-2
• milli (m) 10-3
• micro (m) 10-6
• nano (n) 10-9
• pico (p) 10-12

12
Derived Units Volume (length) x (length) x
(length) (length)3 m x m x
m m3
cm x cm x cm cm3 mL
dm x dm x dm
dm3 L Force mass x acceleration ma
F kg x
newton Energy force x distance mass
x acceleration x distance mad E
newton x m kg x
x m joule