By LeeAnn Kruis. Chemistry Chemistry is stuff such as water(H20), clothes, air, and so on, that has states of matter. The three states of matter is Solid,

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Presentation transcript:

By LeeAnn Kruis

Chemistry Chemistry is stuff such as water(H20), clothes, air, and so on, that has states of matter. The three states of matter is Solid, Liquid, and Gas. Solid has fixed volume and shape that results from the way their particles are arranged. Liquids have fixed volumes but not a fixed shape, because the particles are lose enough to slip past each other. Gas has neither a fixed volume and a fixed shape, the particles are very spaced apart and the particles have weak attractions and hardly touch each other.

Physical and Chemical Changes Physical Changes Physical changes are changes in which the identity of a substance does not change. But the arrangement, location, and speed of the particle may change. Such as in sweet ice tea; dissolving sugar in tea is a physical change.

Chemical Change A chemical change is where the substances change and new substances form. Such as Mercury(II) Oxide, when exposed to heat, the mercury becomes and liquid, and the oxide becomes oxygen gas.

Matter Matter is anything that has mass and volume, such as a balloon, when blowing up the balloon the mass and volume changes due to adding carbon dioxide, or helium.

Mass Mass of an object is the quantity of matter contained in that object. Such as a marble verses a ping-pong ball. The marble has more volume then the ping-pong ball due the marble not having a cavity, such as the ping- pong ball.

Volume Volume is the space the object occupies. An example of space is a text book, the book takes up space due to the volume of it. The volume of the book can be found for multiplying the book’s length times the width, times the height.

Measuring Mass and Volume How you measure mass is with the objects gravitational pull; you usually weigh it in grams. How you measure volume is using liters; you usually fill any beaker to a certain point with water, record the height, and then add the object and record the new height of water; and then you take the difference and find out how much volume the object has.

Density/Weight The weight is defined as the force produced by gravity acting on mass. An example is sand compared to dirt. The dirt will weigh more then the sand because the dirt has a lot more gravitational pull then the sand.

Calculating Density You find the mass and the volume. After you find those you divide them together to get the density.

SI Units; fundamental and derived units; metric prefixes. SI Units are Length(meter), Mass(kilogram), Time(second), Thermodynamic temperature(kelvin), Amount of substance(mole), Electric current(ampere), and Luminous intensity(candela). The last two in the SI Units have very little to do with chemistry, but the first five are very important in the foundation of all chemical measurements.

Converting between units Let’s say you want to convert liters into milliliters. How you would do that is you need to find how many milliliters are in liters.(1000 ml/1L) You then calculate and cancel out the liters to get 0.851L*1000Ml/1L=851Ml.

Chemical and physical properties of matter The physical properties of matter is how a substance looks, and can always be determined without changing the nature of the substance. You can use sucrose(sugar) as an example; Sucrose is solid and white at room temperature, so color and state are physical properties.

Chemical Properties Chemical properties can be identified y trying to cause a chemical change, such as a rusty nail; the reason the rusty nail is rusty is because it’s been exposed for a long period of time to oxygen and a chemical reaction occurs.

Atoms Atoms are in everything around you, air, plants, water, and people. All mater is composed of 110 different kinds of atoms. Atoms can be pure substances, copper, bromine, carbon dioxide, each of these pure substances are elements. Elements can only contain one kind of atom, unless it is a molecule. A molecule is two atoms combined in a definite ratio.

Compounds, and Mixtures Compounds are pure substances that are not elements. An example of a compound is mercury(II)oxide. Mixtures are two or more pure substances. Most foods we eat are mixtures. There are two kinds of mixtures, Homogeneous and Heterogeneous. Homogeneous is a mixture that has two or more pure substances in it, but we can’t see them. Heterogeneous is a mixture that you are able to see the different substances.

Measurements and Calculations in Chemistry Accuracy is how close you estimated the true value to be. Accuracy is important in chemistry because in labs you need to be the closest possible unit to the actual value.

Presision Precision is how closely several measurements that are of the same quantity and that are made in the same way agree with one another.

Rules for Determining Gather the information Plan your work Calculate Verify your results

Significant figures Significant figures are the figures used to measure or calculate an object with certainty.

Converting You sometimes need to convert in chemistry, so you need to know how to convert. Let’s say you want to convert liters into milliliters. How you would do that is you need to find how many milliliters are in liters.(1000 ml/1L) You then calculate and cancel out the liters to get 0.851L*1000Ml/1L=851Ml.(taking from slide 10)

Scientific Notation In scientific notation, exponents are count values; in chemistry you use scientific notation with extremely large numbers and extremely small numbers. Scientific notation has two parts; the first part is with a number, any number, from one to ten, this may be in a decimal form. The second part is to the power of ten. An example is ^6