Evidence of Physical verses Chemical Change

Evidence of Physical verses Chemical Change

verses Chemical Change VOCABULARY physical properties, chemical properties, physical change, chemical change, chemical reaction, Law of Conservation of Mass

Physical Properties All matter has both physical and chemical properties useful to scientists in the classification of it. Typical physical properties we will consider are: color, odor, density, hardness, solubility, phase

of matter, melting points or boiling points. Chemical Properties These are determined by the reactivity of a substance with another substance. Examples: acidity or basicity

reactions with oxygen or other gases What properties cause A to react with B to possibly form AB? Caution: do not get hung up on the nuisances between these two. Simply refer to the definition as defined here in class.

Physical Change This occurs if the shape, size or physical state is changed, but the chemical composition remains the same. (reaction)

any change that results in the formation of new chemical substances. At the molecular level, chemical change involves making or breaking of bonds between atoms. Ex: iron rusting (iron oxide forms) Note: All chemical changes are also physical changes

Reaction Signs of chemical change are: 5 examples change in color (pigmentation loss or gain) rust formation (oxidation of some metals) bubbling or fizzing (gas being produced)

light or heat produced (release of energy) formation of a solid (called a precipitate) Mass Mass or matter can never be destroyed or created during a chemical reactions or

physical change. Mass of all substances present before a chemical change is equal to the mass of all new substances produced after the chemical change. History of the Law of the Conservation of Mass

The ancient Greeks first proposed the idea that the total amount of matter in the universe is constant. Later, Antoine Lavoisier described this with The Law of Conservation of Mass as a fundamental

principle of physics in 1789. He demonstrated it with the following History of the Law of the Conservation of Mass The heating of mercury (Hg) liquid causes it to

react with oxygen forming mercury calx (HgO). The reaction is reversible too. Heating HgO produces O and Hg. Lavoisier was able to account for all mass on either side of the reactions

Law of the Conservation of Mass Mr. Bozeman Conservation of Atoms https://youtu.be/4a2PKulH1So min 0 3

VIDEO LINKS Physical and Chemical Changes - Mr. Bozeman (11min) https://youtu.be/X328AWaJXvI Physical Vs. Chemical Changes - Explained https://youtu.be/4ZGULLWEy1c

verses Chemical Change VOCABULARY physical properties, chemical properties, physical change, chemical change, chemical reaction, Law of Conservation of Mass

Physical Properties All matter has both physical and chemical properties useful to scientists in the classification of it. Typical physical properties we will consider are:

color, odor, density, hardness, solubility, phase of matter, melting points or boiling points. Chemical Properties These are determined by the reactivity of a substance with another substance. Examples: acidity or basicity

reactions with oxygen or other gases What properties cause A to react with B to possibly form AB? Caution: do not get hung up on the nuisances between these two. Simply refer to the definition as defined here in class.

Physical Change This occurs if the shape, size or physical state is changed, but the chemical composition remains the same. (reaction)

any change that results in the formation of new chemical substances. At the molecular level, chemical change involves making or breaking of bonds between atoms. Ex: iron rusting (iron oxide forms) Note: All chemical changes are also physical changes

Reaction Signs of chemical change are: 5 examples change in color (pigmentation loss or gain) rust formation (oxidation of some metals) bubbling or fizzing (gas being produced)

light or heat produced (release of energy) formation of a solid (called a precipitate) Mass Mass or matter can never be destroyed or created during a chemical reactions or

physical change. Mass of all substances present before a chemical change is equal to the mass of all new substances produced after the chemical change. History of the Law of the Conservation of Mass

The ancient Greeks first proposed the idea that the total amount of matter in the universe is constant. Later, Antoine Lavoisier described this with The Law of

Conservation of Mass as a fundamental principle of physics in 1789. He demonstrated it with the following History of the Law of the Conservation of Mass The heating of mercury (Hg) liquid causes it to

react with oxygen forming mercury calx (HgO). The reaction is reversible too. Heating HgO produces O and Hg. Lavoisier was able to account for all mass on either side of the reactions

Law of the Conservation of Mass Mr. Bozeman Conservation of Atoms https://youtu.be/4a2PKulH1So min 0 3

VIDEO LINKS Physical and Chemical Changes - Mr. Bozeman (11min) https://youtu.be/X328AWaJXvI Physical Vs. Chemical Changes - Explained https://youtu.be/4ZGULLWEy1c

Evidence of Physical or Chemical Changes Lab 1. Read and highlight pg 1 2. Complete Physical Properties notes pg 2 3. Complete hands on portion of lab 4. Complete pg 3 prep. Reference reading

pg 1 to find the answers. Physical Properties Baking soda: NaHCO3 solid powder, fine, white Vinegar: CH3COOH (acetic acid)

liquid transparent, clear, sour acidic odor acid Baking Soda & Vinegar 1. Observe the physical properties of baking

soda and vinegar. Record observations. 2. Put 1 spoonful of baking soda into the petri dish. 3. Place a pipette full of vinegar onto baking soda in the petri dish. 4. Observe and record any changes

Physical Properties Corn Starch: NaHCO3 solid powder, fine, white Iodine (povidone-iodine): I-NCHOCH2 liquid - colloid, opaque, brownish/red tint Water: H2O - liquid, transparent, polar, wet

Cornstarch, Water and Iodine 1. Observe the physical properties of cornstarch and iodine. Record observations. 2. Put 1 spoonful of cornstarch into water. Stir 3. Using the dropper, drip one drop at a time of

iodine into the mixture and stir after each. 4. Observe and record any changes Physical Properties Epsom salts : MgSO4 magnesium sulfate solid -coarse, crystalline white w/ blueish

tinge https://youtu.be/TOllLQSzzGI - washing soda : Na3CO3 (sodium carbonate)

solid - powder pale white to yellowish tint Water: H2O - liquid, transparent, polar, wet Epsom Salt, Washing soda and water in solution

1. Observe the physical properties of Epsom Salt and Washing soda . Record observations. 2. Put 1 spoonful of each into water. Stir 3. Then pipette several samples of each onto a petri dish. 4. Observe and record any changes

Physical Properties Copper penny: Cu . CuO2H solid metallic, Abe Lincoln, patina or tarnish greenish tinge Table Salt: NaCl

solid - crystalline granular, cuboidal, white Vinegar liquid, transparent, clear, sour acidic odor Sugar and Water 1. Observe the physical properties of

sugar and water. Record observations. 2. Put 1 spoonful of sugar into water. Stir 3. Observe and record any changes Physical Properties Sugar : C6H12O6

solid solid, granular crystalline, pale white Water: H2O - liquid, transparent, polar, wet Form a solution observe

Physical Properties https://youtu.be/MEvYVxXHEGY?t=60 Steel wool: (Iron)Fe solid - metallic, fibrous, luster, some

shine Vinegar (acetic acid) liquid, transparent, clear, sour acidic odor

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