Final Integrative Guide OT24 - Daphne Cepeda PDF

UNIVERSIDAD DE MONTERREY VICERRECTORÍA DE EDUCACIÓN MEDIA SUPERIOR NATURAL SCIENCE ACADEMY CLU: INTRODUCTION TO EXPERIMENTAL SCIENCES FI...

UNIVERSIDAD DE MONTERREY VICERRECTORÍA DE EDUCACIÓN MEDIA SUPERIOR NATURAL SCIENCE ACADEMY CLU: INTRODUCTION TO EXPERIMENTAL SCIENCES FINAL SUMMARIZED ACTIVITY Name: Daphne Michelle Cepeda Salinas ID: 661112 Date: November 22, 2024 Classroom: 3304 The following activity is considered a summarized guideline of the topics covered in the semester, but a full comprehensive study of each topic should be performed by the student. Topic 0. Scientific method. 1. Define the following concepts. Scientific investigation: Is a deliberate search for knowledge through the application of certain methods and principles; a plan for asking questions and testing possible answers. Scientific method: It is an organized process, a series of steps that scientists use to solve investigation problems. Hypothesis: Make a statement based on the question and data collected. Observation: collect information Qualitative data: Information that describes color, odor, shape, or other physical characteristics (involves the use of senses). Quantitative data: Answers the question “How”: How much does it weight? How high is it? How long will it take? Anything that refers to measurable quantities, and has units and uncertainty. (Involves the use of measuring devices). Topic 1.1 and 1.2 Nuclear Atom 1. According to the atomic model, state the subatomic particles, and identify the symbol to represent each one of them and its charge. Proton (p+): has positive charge. Electron (e-): Has a negative charge and its mass is extremely small. It moves around the nucleus in defined spaces called orbitals. Neutron (n°): Subatomic particle which has no electric charge (it is neutral). Nearly equal to the mass of a proton. The nucleus is composed by neutrons and protons 2. Define the following laws and/or principles and indicate the name of the scientist who proposed them. Scientists that Law or principle Definition proposed it “Mass cannot be created Lavoisier Law of or destroyed, it is merely conservation of rearranged”. mass “A chemical compound Joseph Proust always contains exactly Law of definite the same proportion of proportions elements by mass.” “States that we cannot Werner know both the position and Heisenberg trajectory of an electron, with perfect accuracy; the Uncertainty more we nail down the principle electron’s position, the less we know about its trajectory and vice versa.” Topic 1.3 Periodic Table 1. Answer the following exercises: a) It states that atoms lose, gain, or share electrons to acquire a complete set of eight valence electrons (stable electronic configuration of a noble gas) ___Octet rule__ b) It is the force, the power of an atom to attract electrons towards itself ___electronegativity____ c) It corresponds to the number of protons of the element ___Atomic number____ d) Corresponds to the weighted average of the masses of the isotopes of that element ___Atomic mass____ e) They indicate the energy levels occupied by the valence electron of an element. (Horizontal rows) __Periods____ f) They indicate the number of valence electrons of an element ___Groups_____ g) They are the electrons found in the last energy shell __Valence electrons__ 2. Make a table where you distinguish characteristics of metals, nonmetals and metalloids and mention examples of each Metals Nonmetals Metalloids - Shiny solids at room - They are generally - Exhibit physical and temperature. gases or brittle solids of chemical properties that - They can be shaped an opaque appearance, are typical of both into wires (ductile) or and bad conductors of metals and nonmetals. hammered into flat heat and electricity. - They are mostly used to sheets (malleable) - They are not malleable build technological - They are good nor ductile. components such as conductors of heat and - The only liquid chips for computers. electricity. non-metal is bromine - They are - They typically have high (Br). semiconductors. melting points and high - They typically have low densities. melting points and low - They usually have 1, 2 densities. or 3 valence electrons - They have 5, 6 or 7 and for this reason they valence electrons so tend to lose them when they accept electrons they are combined with when they are another element. chemically combined with other element. Ex: Ex: Ex: Gold, Silver, Aluminum, Hydrogen, Helium, Carbon, boron, silicon, germanium, Copper, Iron, Nitrogen, Oxygen arsenic 3. Identify the name of the concept that corresponds each arrow: 4. According to the Atomic mass and the atomic number calculate the number of neutrons found on the element. 209.98 - 85 =124.98 or 125 neutrons  5. Identify the name, groups in the periodic table, level in the periodic table, valence electrons, atomic number, and atomic mass of the following elements. Name Group or Period Valence Atomic Atomic Mass family Electrons Number O Oxygen 16 2 6 8 15.99 Li Lithium 1 2 1 3 6.94 F Fluorine 17 2 7 9 18.998 Mg Magnesium 2 3 2 12 24.305 Ar Argon 18 3 8 18 39.948 Topic 1.4 Electron Configuration 1. Determine the electron configuration of the following elements and identify the element, also mention the group and the period to which it belongs. Z= 12 Name of the element: Magnesium Electron configuration Electron distribution Group/family 2 Period 3 Valence Electrons 2 Z= 5 Name of the element: Boron Electron configuration Electron distribution Group/family 13 Period 2 Valence Electrons 3 Z= 19 Name of the element: Potassium Electron configuration Electron distribution Group/family 1 Period 4 Valence Electrons 1 Z= 35 Name of the element: Bromine Electron configuration Electron distribution Group/family 17 Period 4 Valence Electrons 7 Z= 18 Name of the element: Argon Electron configuration Electronic distribution Group/family 18 Period 3 Valence Electrons 8 Z= 32 Name of the element: Germanium Electron configuration Electronic distribution Group/family 14 Period 4 Valence Electrons 4 2. Outline the principles of Aufbau, Pauli exclusion principle, and Hund Rules. Aufbau Principle: electrons will occupy the lowest energy level possible, and “build up” to higher energy levels. Pauli Exclusion Principle: No two electrons can share the same combination of the four quantum numbers. Since only 2 electrons may occupy an orbital, they must have opposite spin (clockwise & counterclockwise). Hund's Rules: when filling a sublevel, such as 3p, e- will go to an empty orbital prior to pairing up (spread out before pairing up). Topic 1.5 Chemical Bonds 1. Compare and contrast the covalent bond and the ionic bond. Include two examples of each. Compare Both of them are types of bonds between elements. Both of them allow the formation of chemical compounds. Both of them want to obtain 8 valence electrons in order to complete their octet rule. Contrast Ionic compounds Transfer of electrons Metal + Nonmetal High mp/bp Solid at room T Example: NaCl Conduct electricity. Examples: NaCl, sodium chloride Na2O, sodium oxide Covalent compounds Sharing electrons Nonmetal + nonmetal Molecular (low mp/bp) Liquid or gaseous at room T Example: CO2, Cl2 Non conductors of electricity. Examples: hydrogen, nitrogen Topic 1.6 Introduction to Carbon Chemistry 1. Outline the importance of carbon as the element of life. It is the basic element of life in organic chemistry; the basic element in the formation of biomolecules: Carbohydrates, lipids, proteins, nucleic acids 2. Distinguish between organic and inorganic compounds, and give examples of each. Organic Chemistry: It is the study of the carbon compounds. Compounds from animals or vegetables containing carbon and previously thought to contain a vital force for living cells. (Except: CO2, CO, Carbonates and bicarbonates) Examples: carbohydrates and proteins. Inorganic Chemistry: It is the study of compounds that don’t contain carbon. Compounds made of different elements, most of them do not contain carbon. Water is the most abundant compound of the group. Examples: Table salt (NaCl) and water Topic 1.7 Hydrocarbons 1. Complete the following chart: Hydrocarbons Bonds General formula Ending Alkane single CnH2n+2 -ane Alkenes (olefins) double CnH2n -ene Alkyne Triple CnH2n-2 -yne 2. State the name of the following hydrocarbons according to the number of carbons. Use the general formulas for each type of hydrocarbon. Number of carbon Alkanes Alkenes Alkynes atoms 1 C1H3 C1H1 C1H-1 - Methane - Methene - Methyne 2 C2H6 C2H4 C2H2 - Ethane - Ethene - Ethyne 3 C3H8 C3H6 C3H4 - Propane - Propene - Propyne 4 C4H10 C4H8 C4H6 - Butene - Butyne - Butane 5 C5H12 C5H10 C5H8 - Pentane - Pentene - Pentyne 6 C6H14 C6H12 C6H10 - Hexane - Hexene - Hexyne 7 C7H16 C7H14 C7H12 - Heptane - Heptene - Heptyne 3. Determine the name of the hydrocarbons below: 2-Heptyne 2, 3 dimethylheptane 3, 3 diethyl, 8, methyl nonane Topic 1.8 Functional groups 1. Define what a functional group is. An atom or group of atoms that give the compound specific characteristics, they are significant because they’re the reactive part of the molecule and frequently dictate the chemical properties of the compound. 2. Complete the following table, and draw the functional groups that they ask of you. Common name functional group Carbonyl RCHO Carboxylic acid R-COOH Amino NH2 Amides R-CONH2 Alcohol OH Esters R-COOR 3. Draw and label at least 2 examples of molecules where we can find a functional group Proteins and carbohydrates INFORMATION ANALYSIS Use the following information to answer the given questions. Sodium chloride, or salt, contains 40% sodium. Therefore, 1 gram of salt contains 400 milligrams of sodium, so our daily intake can reach 4,800 milligrams. Our body needs only a small amount of sodium for functions such as the nervous system, muscle contraction, and water balance within cells. Given this information, a study was conducted on people aged 16 to 36 years. Some of the most commonly consumed foods in their daily diet were collected to identify those with the highest sodium content and to raise awareness about reducing sodium intake to prevent systemic diseases. Graph 1. Sodium content (mg) in 10g of different types of food. 1. State the independent variable. Types of food 2. State the investigation question for this research case Will there be a difference on the amount of sodium (mg) in different daily types of food? 3. Suggest a hypothesis for the investigation question. There will be a significant difference in the amount of sodium between the 6 foods tested.  4. Calculate the Sodium content (mg) difference between the Chicken Broth cube and the Oreo Cookies. 6.6mg - 4.3mg = 2.3mg there are 2.3mg of difference between the Oreos and the Chicken Broth REFERENCES Alroys Sheet Metal & Fabrication. (2022, diciembre 19). Different types of metals & their applications - Alroys. https://alroys.com/different-types-of-metals-and-their-applications/ BYJUS; BYJU’S. (2016, enero 11). Non-metals. https://byjus.com/chemistry/non-metals/ Chemistry LibreTexts. (2015, septiembre 27). 3.5: Ionic compounds- formulas and names. Libretexts. https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_A_Molecular_Approach_(T ro)/03%3A_Molecules_Compounds_and_Chemical_Equations/3.05%3A_Ionic_Compounds-_Form ulas_and_Names Encyclopedia Britannica. (2024). Covalent bond. En Encyclopedia Britannica. Study.com. (s/f). No title. Recuperado el 30 de noviembre de 2024, de https://study.com/academy/lesson/metalloid-elements-on-the-periodic-table-definition-propertie s.html "This is my own work and was carried out in strict adherence to the honor code; any text or reference that was not of my authorship is cited, including sources extracted using artificial intelligence. I am aware that any academic dishonesty is graded with zero and the protocols apply according to the Academic Integrity Committee of Prepa UDEM." Signature: Daphne Michelle Cepeda Salinas