CHEM 101 1st EditionExam # 1 Study GuideStates Of Matter1. If it is rigid, and has a volume that is unchangeable then it is __________2. If it has no permanent shape and doesn’t necessarily fill a container then it is _________3. If it has no permanent shape but expands to fill the container than it is _________ Pure Substances and Mixtures1. Pure substance simply means that it is a ,substance or material, that contains only one type of building block- meaning that the only pure substances are elements and compounds. As defined in class a pure substance cannot be further purified. A compound can be chemically broken down into elements, but it is completely purified whether a compound or element.2. There are two types of mixtures: Homogenous Mixture and Heterogeneous Mixture. Homogeneous mixture: is a mixture made up of substances that cannot be easily separated easily- examples sugar water, coffee and creamerHeterogeneous Mixture: is a mixture that is easy to separate: Ex: such as rocks, pizza ( as in the ingredients in the pizza; cheese, sauce, pepperoni) cereal and milkNaming Elements1. There are a lot of elements that are easy to name such H=Hydrogen, O= oxygen , and He= Helium. But there are some elements that trick you. Such as Ag=Silver Au= Gold K=potassium, Na=Sodium, Hg=Mercurya. These are just a few different ones I believe will be on the testb. But definitely review the periodic table!Terms Needed to Know1. Atom: the atom is THE smallest part of an element containing the chemical properties of the element. Has the nucleus and the protons, neutrons, and electrons. The number of protons determine the type of element2. Molecule: this is the part of the compound that is the smallest unit that still has chemical characteristics-3. Ion: an Ion is when an element loses or gains an electron. The element will never have a change in protons but it will sometimes loss or gain electrons4. Formula Unit: is from an ionic compound , does not form a molecules, the formula with the smallest amount of elements out the whole formula.5. Compound: a pure substance composed of two or more elements chemically joinedtogether6. Element: a substance that cannot be broken down anymore chemicallyElectrons, Protons, and Neutrons1. Protons: a particle, that is the lightest and the most stable, that is part of an element and generally has the same amount as there are electrons. The number of protons determines the type of element.2. Neutrons: a particle that has no charge, weighs slightly more than a proton and is present in the nucleus with protons3. Electrons: a particle with a negative charge, usually matches the number of protons, exists independent of the nucleus, aka orbits the nucleus rather than beinginside it like protons and neutrons.4. General make of a nucleus:i. Atoms and protons inside the nucleus with positive an neutral charges, and the electrons orbit the nucleus with a negative chargeIsotopes:1. Isotope: has an equal number of protons and electrons, thus they have the same atomic number and the same chemical reactions. Now with carbon, a normal carbon also has 6 neutrons in it's nucleus. It's atomic weight is mostly the weight of the protons and neutrons, so it's weight is 6 protons+ 6 neutrons = 12 atomic weight 2. Neutrons have no charge, so there is nothing in the nucleus that wants to kick themout or chase electrons away. 3.4. An isotope is just any normal element like carbon 12 but where you add or subtract neutrons. If you added two neutrons to carbon 12 it would be now carbon 14 atomic weight and it would be an isotope of carbon12 (normal carbon).a. Element Symbol Mass Abundance Symbol Mass Abundance5. Carbon C(12) 12.000000 98.90 C(13) 13.003355 1.10 6. Nitrogen N(14) 14.003074 99.63 N(15) 15.000109 0.37 7. Oxygen O(16) 15.994915 99.76 O(17) 16.999131 0.038Terminologies of the Periodic Table1. Groups: there are 18 and they count horizontal to the periodic table. For example a popular group are the Noble Gases: Argon( Ar) Xenon(Xe), Helium (He), Neon (Ne) Krypton (Kr) and Radon (Rn). These elements were GROUPED together because they are extremely stable they do not want to combine with another element. Another groups is called Akali Metals . they are the first group on the Periodic Table on the left. These elements are grouped together because they barely have the characteristics of a metal and they are sometimes classified as non-metals2. Periods: there are 7 and they count vertically. The period number of an element signifies the highest unexcited energy level for an electron in that element. The number of elements in a period increases as you move down the periodic tablebecause there are more sublevels per level as the energy level of the atom increases.3. Metals: Mostly make up the periodic table from Lithium (Li) down to Francium(Fr) all the way to Aluminum(Al) stair stepping down to Germanium(Ge) Antimony(Sb) Polonium(Po) Metals are metals because these elements conduct electricity4. Nonmetals: The term "nonmetals" is simply used to classify hydrogen (H), carbon (C), nitrogen (N), phosphorus (P), oxygen (O), sulfur (S) and selenium (Se).5. Metalloids: The metalloids are boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te) and polonium (Po). They sometimes behave as semiconductors (B, Si, Ge) rather than as conductors. Metalloids are also called "semi-metals" or "poor metals."Differences between Ionic Compounds and Molecular Compounds1. Ionic Compounds: Ionic compounds involve ions, so they are typically the combination of a metal and a nonmetal, such as NaCl, CaBr2, AlCl3, etc. Some ions that are made completely of nonmetal can form ionic compounds. The main example is the ammonium ion, NH4+2. Molecular Compounds: Molecular compounds always involve two nonmetals, CO, CO2, NH3, N2O4, etc. That is how you can identify them easily, the bonding does not involve ions at all, so they are nonconductors of electricity under any circumstancei. Monoatomic Ions3. H+ hydrogen ion H- hydride4. Li+ lithium ion F- fluoride5. Na+ sodium ion Cl- chloride6. K+ potassium ion Br- bromide7. Rb+ rubidium ion