2.6 chem

14.1

Week 1: Introduction to Chemistry, Matter and Measurements

Polyatomic Ions AP Chemistry

YR 11 CHEM Term 3 Assessment - Prelims Content

Organic Chem

Organic Chemistry Chapter 2

Organic Chemistry - Functional Groups

Chem 3A Fuctional Groups

KSU chem ch1

Physics and Chemistry Definitions, Laws, and Principles

Clinical Chemistry and Laboratory Quality Management Flashcards

Chemistry

Gen chem chapter 2

CHEM 115 quiz 1

Chemistry AS definition

Chemistry Reactions and Solutions

Biochemical Interactions and Water Chemistry

CHEMISTRY Chemistry is the study of matter . -It's composition structure, and properties -The process it goes through and the energy changes that occur Matter is anything that has mass and volume. -Mass= a measure of the amount of matter -Volume=a measure of how much space something takes up Everything is made of matter Atoms are the building blocks of matter. Atom= the smallest unit of an element that maintains the identity of the element. Exmaple= atmospheric nitrogen, N2 conatins 2 atoms of the element nitrogen. Element= a pure substance that cannot be broken down into simple and more stable substances(elements). Example= anything in the periodic table. Compound= a pure substance that can be broken into simple and more stable subtances(elements) Made from chemmically combining atoms of two or more elements. Example=H2O Matter Substance Mixture Element compound homogeneous. heterogeneous Subtances= pure -Fixed composition throughout -Same properties througNaCI, C6H12O6 Element = form of matter -on the periodic table -cannot be broken down into anything simplier or more stable -exist naturally as 1 atom(monoatomic) or two atoms Examples= C, O2, something Compounds= chemically combined atoms of 2 or more different elements. Fixed proportions, written as a formula. -Can be chemically broken into simplier and more stable subtances(elements) -Have different properties as a compound than the parts that make it up Example= NaCI, CO2, C6H12O6 Mixtures= combination Variable composition throughout Each component retains its unique properties. -Mixtures can be separated into substances -Examples= salt water, lemonde, blood, air Homogeneous mixture= even destribution" same" -Appears blended -can be physically broken down into different components -Solution: one subtance(solute) is dissolve into another(solvent) -Aqueous solution= when the solute is dissolved into water -Alloy: A sollution of metals -Examples: Lemonade, stainless steel. Heterogenous mixture: Uneven destribution" different" -Can be physically broken down into different components and often easily -components can often be seen or seperated out over time. -Examples: Salad dressing, paint, blood. Properties Extensive: depends on the amount of matter that it presents -Ex. Mass, volume, amount of energy, ect. -Aluminum can have a mass of 10g or a mass of 200g based on how much you have. Intensive= do not depend on the amount of matter that is present -ex. Density, melting point, boiling point, specific heat, ect. -Aluminum always has a density of 2.7 g/cm to the power of 3, regarless of if you have a few pieces versus giant sheets. Physical= can be observe without changing the identity of the subtance -ex. Density, boiling point, state, color -State of matter -solid: definite volume and defined shape -liquid: definite volume and undefined volume -Gas: Indefinite volume and indefinite volume. Chemical: Can be only be observed by changing the compositions/identity of the subtance. -ex. Reactivity, ability to decompose, instability. Physical changes: Chages in the substance that doesn't chnage its density -ex. Boiling, melting, dissolving, vaporizing, cutting. Chemical changes: Chance of a substance into another substance; when a chemical reaction occurs. -ex. Burning, oxidation, rotting, corroding, fermenting -chemical changes do not have a change in amount of mass/matter -law of conservation of matter: matter is never created or destroyed, it only changes form -chemical changes always cause a change in composition. Evidence of chemical reacton: -Release of light -sudden tempeture change -sudden color change -odor change -gas given off -sudden apperance of a solid -this solid that forms is known as a precipitate.

polymers chem