Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous...
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Transcript of Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous...
![Page 1: Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno.](https://reader033.fdocuments.us/reader033/viewer/2022061514/56649ea85503460f94bab460/html5/thumbnails/1.jpg)
Matter Flowchart
MATTER
Can it be physically separated?
Homogeneous Mixture
(solution)
Heterogeneous Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be chemically decomposed?
noyesIs the composition uniform?
noyes
![Page 2: Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno.](https://reader033.fdocuments.us/reader033/viewer/2022061514/56649ea85503460f94bab460/html5/thumbnails/2.jpg)
A. Matter Flowchart
Examples:
graphite
pepper
sugar (sucrose)
paint
soda
element
hetero. mixture
compound
hetero. Mixture
Solution(homogeneous mixture)
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C. Johannesson
Pure Substances
Element composed of identical atoms EX: copper wire, aluminum foil
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Pure Substances
Compound composed of 2 or more elements
in a fixed ratio
properties differ from those of individual elements
Chemically combined and must be chemically separated
EX: table salt (NaCl)
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Mixtures
Variable combination of 2 or more pure substances.
Physically combined and separated
Heterogeneous Homogeneous
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Mixtures
Solution homogeneous very small particles no Tyndall effect Tyndall Effect
particles don’t settle EX: rubbing alcohol
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What are the differences between an element, compound and mixture?
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Matter has properties
Two basic types of properties that we can associate with matter.
Physical properties
Chemical properties
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Physical Properties
Anything that can be observed without changing the identity of the substance. (Tends to be measurable.)
• melting point• boiling point• electrical conductivity• color
• density • thermal conductivity• ductility• malleability
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Chemical Properties
The way a substance may change or react to form other substances
• heat of combustion• reactivity with water• PH• Oxidation• Flammability
• Reactivity to other chemicals
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Physical Changes
Do NOT CHANGE THE TYPE OF MATTER
Nothing new or different is formedCould be a change in:
Mass Volume Density Change in state Color Shape
Size
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Examples of Physical Changes
Boiling Freezing Dissolving Breaking Making a mixture
2 or more types of matter (substances) mixed together Not in specific amounts Can be separated physically
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Chemical Changes
The composition of the substance changes.
The substances present at the beginning of the change are not present at the end; new substances are formed. The change cannot be “undone.”
Picture from www.chem4kids.com
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Chemical Changes
Evidence of a chemical reactionFormation of gas Formation of precipitate Change in color Change in energy
Endothermic Absorbs heat energy (gets cold) Exothermic Releases heat energy (gets hot)
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Chemical Changes
Atoms are re-arranged, NOT created or destroyed
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Law of Conservation of Matter
Matter is conserved type of atoms does not change
Nothing is created or destroyed
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Atoms and Ions• An atom has a zero net charge• How does an ion become an atom? Loses
Electrons• What element am I?• Protons=8 Electrons=8 Neutron=9• Are these the same element?• Proton = 9 Electron =10 Neutron = 10• Proton = 9 Electron=9 Neutron = 11
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Part 2 Notes: Compounds• Noble gases-located… Right most column of the PT• They are the only elements that tend to exist …as
isolated atoms• Molecule: the smallest electrically neutral unit of a
substance that still has properties of that substance; two or more atoms that are covalently bonded and act as a single unit
• Diatomic molecule: molecule made of two atoms
• H2 O2 F2 Br2 I2 N2 Cl2 (At2)
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Molecular or covalent compounds: compounds composed of neutral molecules
• Relatively low MP and BP (below 300°C)• Exits as gases or liquids because of low BP/MP• Composed of generally 2 or more nonmetallic
elements• The smallest unit is a molecule
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Ions: atoms or groups of atoms that have a positive or negative charge
• Ionic compounds: compounds composed of two or more ions that have opposite charges
• MP and BP: fairly to very high• Exists as solid crystals• Composed of a metallic ion with a nonmetallic
ion in a ratio where there is a balance of opposite charges
• Smallest unit called formula unit (do not abbreviate)
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• Chemical formula: shows the kinds and numbers of atoms in the smallest representative unit of the substance
• Molecular formula: shows the kind and numbers of atoms present in one molecule of the substance
• Formula unit: smallest whole number ratio of positive and negative ions in the smallest electrically neutral portion of a compound which is ionically bonded
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Pure Substances
Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.
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Pure Substances
For example…
Two different compounds, each has a definite composition.
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Law of Definite proportions-does not depend on the amount of substance
• Example: Given the formulas CO and CO2, what do you know about these compounds based on the Law of Definite proportions? The ratio of C to O within each compound will be constant-but it will be different from one compound to another
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Example 1:
• Compound A: 2.41gC = 0.748 gC/gO 3.22g O
Compound B: 6.71g C = 0.375 gC/gO 17.9g O
A:B 0.748 gC/gO = _2_ 0.375 gC/gO 1 The mass ratio of C per gram of O in compound A to that of compound B is 2:1
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Or…
H2O and H2O2
H:O H:O 2:1 2:2 2g:16g 2g:32g
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Example 2
N:O is 7:468g of N+O – 42g of N = 26g of O
N:O is 42g/26g so 1.6gN per gram of O
No, this is not nitrous oxide since it is not in a 7:4 mass ratio