alund lab 3

Lab 3: Introduction to the Periodic Table Autumn Lund 16 June 2022 Location: Home CHE 1111 C02 Lab Partner: N/A

Lab 3: Introduction to the Periodic Table Exercise 1 1. Describe how the properties of the different types of elements (metals, nonmetals, metalloids) differ. (Make sure to use your own words.) - For metals, they are distinguished by their hardness because they cannot be easily broken or torn apart. Metals also have a higher density in in which a smaller size piece of metal can have more weight than compared to other elements, as well as shiny surfaces which is known as their luster. Metals are also insoluble and corrode when exposed to air. They can also conduct electricity better thank any element and they have high melting points (Ranga.nr, 2022). - Non metals are dull, have low melting points, poor electric conductors, as well as poor heat conductors. Unlike metals, nonmetals have a low density and are very brittle. Nonmetals are more electronegative which allows them to attract more electrons as well as have a strong hold of the electrons they already have (Admin, 2022). - Because metalloids are a medium mix between metals and nonmetals, their properties are similar between both distinct categories. Just as metals, metalloids have a metallic luster and are solid, however, they are brittle like nonmetals. Their conductivity is a mix because metalloids are semi-conductive, which means they can conduct heat relatively well, but not as strong as metals or as week as nonmetals (Alchin, 2018). 2. Explain what characteristics of metalloids are more like metals and which are more like nonmetals based on the research you conducted and the information recorded in Data Table 1.) - In table one, when comparing the properties, it can be seen that the metalloids fit pretty well throughout the table and that it does not seem like an outlier. The metalloid shared about two of the same properties as nonmetals and those were: neither malleable or ductile and their presence in nature does not occur unless combined. The main property shared with metals was their melting and boiling points. This is because the other properties were mixed between nonmetals and metals. The metalloids conductivity was semiconductive which was between the metals good conductivity and the nonmetals poor conductivity. The metalloid also had some reactivity but not as strong or low as the others. And finally, the electron activity was very similar all throughout because the metalloids could wither lose or gain electrons during a reaction. 3. Define the term “transition.” How does this definition apply to the transition metals? (Make sure to use your own words.) - The word ‘transition’ can be defined as the process of changing from one thing to another. In this case a sort of bridge between the two different sides of the periodic table. The two sides of the periodic table are very different and for one element to essentially ‘transition’ it will need something to help change its state to reach the other side ( Transition definition & meaning, n.d.). Photo 1: Completed Periodic Table Makes sure to sign and date your image and insert below.

Data Table 1: Physical and Chemical Properties of Elements Group Ductile/ Malleable Conductivity Melting & Boiling Points Presence in the Environment Reactivity Electron Behavior Alkali Metal - Na Ductile & malleable Good thermal and electric conductor Low melting and boiling point compared to other metals Does not occur in nature unless combined Highly reactive Ready to lose the single electron in its outer shell Alkaline Earth Metal - Mg Ductile & malleable when heated Good thermal and electric conductor High melting and boiling points Does not occur in nature unless combined Highly reactive In reactions, loses electron(s) Transition Metal - Fe Ductile & malleable Good thermal and electric conductor High melting and boiling point Occurs naturally in nature as pure form (and combined) High reactivity Loses electrons in reactions ( 2 or 3 ) for stable ion Metalloids - Ge Neither malleable or ductile Semi good thermal and electric conductor High melting and boiling point Does not occur in nature unless combined Intermediate reactivity Easily gain or lose 4 electrons in reactions Halogen - Cl Neither malleable or ductile Poor thermal and electric conductor Low melting and boiling point Does not occur in nature unless combined Highly reactive Gains an electron in a reaction Noble gas - Ar Neither malleable or ductile Poor thermal and electric conductor Low melting and boiling point Does not occur in nature unless combined Non-reactive No loss or gain of electrons

Data Table 2: Element Groups and Descriptions Element Group Name Group Number Metal/ Nonmetal/ Metalloid Description Neon Noble Gases 18 Non-metal f) colorless, tasteless, and odorless gas, unreactive, nonconductive Bromine Halogens 17 Non-metal d) not found as a free element (uncombined) in nature, reddish-brown liquid that vaporizes readily at room temperature to a red gas with a strong disagreeable odor Beryllium Alkaline earth metal 2 metal e) Silvery-white, ductile, malleable, conductive solid with a high melting point for this type of element Platinum Transition metals 10 metal b) Silvery white, relatively soft, low density, conductive solid that is not found as a free element in nature but commonly found combined in alloys with copper or nickel Potassium Alkali Metals 1 metal g) soft, easy to cut with a knife to expose a silvery surface that rapidly oxidizes in air; never found uncombined in nature Silicon Carbon group 14 metalloid c) Metallic luster and grayish solid, very common in rocks and gemstones such as amethyst and opal, semiconductor Sulfur Oxygen group 16 Non-metal a) Pale yellow, odorless, brittle solid at room temperature, nonconductor Extension Question Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. Describe how electronegativity is illustrated on the periodic table including trends between groups and periods and significance of atom size. - First electronegativity helps describe how close the electrons will be to the atom. To see this along and through the table, you have to follow the trends. When moving from left to right across the periodic table, the electronegativity increases, however, when you move down along a group within the periodic table, the electronegativity decreases because of the increase in shells around an atom. The farther these shells are from the nucleus, the radius increases meaning the electrons are farther apart ( Electronegativity trend, 2020). Additional Photo Requirements (I was going to insert my HOL in here to but it will not show up at all) References