BSC 181 1st Edition Lecture 3Outline of Last Lecture I. Body PlanesII. Body CavitiesOutline of Current Lecture III. Matter A. Definition of Matter IV. Atoms and Elements A. Definitions of Atoms and ElementsV. Models of the AtomA. Identifying ElementsVI. Mixtures and CompoundsCurrent LectureMatter: is anything that occupies space and has mass. There are three different states of matter known as the solid, liquid, and gaseous states. Solid: has a definite shape, and a definite volumeLiquid: has an indefinite shape, and a definite volumeGas: has an indefinite shape and an indefinite volumeThese forms of matter are comprised of Elements, and these elements cannot be broken down into smaller substances without changing that elements identity. That is, if you break down an element into smaller substances it will not be that element anymore it will be a completely different element. What makes up matter are the elements in it. What makes up the elements are the atoms. Atoms are the unique building blocks of an element. Just like each element has unique physical and chemical properties to it, the atom of that element will have the same physical and chemical properties. Atoms are the smallest form of the elements that have the same properties.Atomic Structure: Atoms are made up of protons, neutrons and electrons. Both the protons andneutrons surround the nucleus of the atom, and because the protons and neutrons are heavier than the electrons, the nucleus is very dense. Because the protons have a positive charge and These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.the neutrons are negative, that makes the nucleus positively charged. However the atom as a whole is neutral. The atom as a whole is neutral because the protons, which are positive, and the electrons, which are negative, cancel each other out to make it neutral. Proton: has a positive charge, about the same mass as a neutron (1 amu) amu stands for: atomic mass unitNeutron: has no charge, about the same mass as a proton (1 amu) Electron: has a negative charge, and while electrons are smaller than the neutrons and protons, its negative charge is equal to that of the positive charge of the proton. Its mass is only about 1/2000 the mass of a proton. Electrons are in orbitals around the nucleus. *I suggest again to look at the visuals provided in the book to get a better understanding of where exactly the electrons are in comparison with everything else.Models of the Atom: There are a few different models that depict the atom. There is the Planetary Model, and the Orbital Model. We still look at and use the planetary model, but only for illustrations. It is an outdated model in terms of showing where the electrons are. You can never really tell where the electrons are in the atom only that they surround the nucleus. So thefact that the planetary model shows the electrons in perfect circular trajectories is incorrect. Which leads to the orbital model which is a more modern model which depicts an electron cloud instead.Identifying Elements: Different elements contain different numbers of subatomic particles, because of this we can identify which elements are which. The subatomic particles are the protons, electrons and neutrons. For example, Hydrogen has one proton, no neutrons, and one electron. So when we see something with one proton, no neutrons, and one electron, we know that is it is hydrogen. However, if you change the amount of protons that are in that element, than you change what that elements is. Which makes sense, if you add a proton to hydrogen so that is has two protons, then it’s not really hydrogen anymore, because hydrogen can only have one proton. However, you can change the amount of neutrons in an element. Changing the neutrons will only change the mass. When you do change the mass by changing the amount of neutrons, then the element is called an Isotope. With isotopes, the only thing that is different from the element is the mass and the amount of neutrons.If we are looking at the periodic table, you can tell how many protons are in an element by looking at the Atomic Number. The Mass Number on the periodic table tells you how many protons and neutrons are in that element. Mixtures and Compounds: Atoms can combine with other atoms to form Molecules and Compounds.A Molecule: is two atoms that are bonded together, the two atoms can be of the same element or they can be two atoms from different elements. For example, H2 (same element), or C2H4O2 (different elements)A Compound: is two or more of the different types of atoms bonded together. For example, C2H4O2Mixture: is when two or more components physically mix together. It is important to note here that it is not completed chemically, it is simply mixing to or more things together. There are three different types of mixtures. They are called solutions, colloids, and suspensions. Solutions: These are homogeneous mixtures, which means that everything is equally dispersed throughout. In solutions, there is the solvent, and the solute(s). The solvent is the substance that is in the greatest amount. It is usually a liquid, and the liquid is usually water. A solute is what you put into the solvent. There can be more than one solute in a solvent. For example, if we have tea, the solvent is going to be the water, and the solute is going to be the tea extract. If you add sugar or cream to your tea, those are solutes as well.Colloid: (also called emulsions) these are heterogeneous mixtures, which means that noteverything is equally distributed throughout. They have large solute particles that do notsettle out. An example of a colloid would be fog. Colloids have a unique property. Some can undergo sol-gel transformation, you can think of it like a jello mold. Before you put jello in the fridge it is more of a liquid substance, but when you take it out after a while ithas become more like a solid. Suspensions: these are also heterogeneous mixtures. The best way to describe these is thought the example of blood. Blood is a suspension, so if you took out a cup of blood and let it sit the heavier stuff will disperse to the bottom. (The large solutes settle to the bottom). The way to tell between a colloid and a suspension is that in a suspension, the large solutes will settle to the bottom when a colloid will not. Milk is a colloid. The fats in