Q2-G9-Science-Module 1 PDF

# Science Quarter 2 - Module 1: Electronic Structure of Matter ## Development Team of the Module ### Writers: - MA. CARMEL M. MACASINAG, Master Teacher I - CARMELITA G. YAP, Master Teacher I - GENOVIE G. TAGUM, Master Teacher II - MYLA JENNIE G. TAN, Master Teacher I - JESSE A. TISTON, Tea...

# Science Quarter 2 - Module 1: Electronic Structure of Matter ## Development Team of the Module ### Writers: - MA. CARMEL M. MACASINAG, Master Teacher I - CARMELITA G. YAP, Master Teacher I - GENOVIE G. TAGUM, Master Teacher II - MYLA JENNIE G. TAN, Master Teacher I - JESSE A. TISTON, Teacher I - IMELDA V. MINGOA, Teacher II - MARITES T. TUDIO, Teacher III - RECHELLE M. CARRIDO, Teacher I - LYDEN B. PAICAN, Teacher I - JOSEPHINE B. HERNANDO, Teacher I - DARIO V. AGAS, Teacher I - DARYL G. GUMACAL, Teacher I - MIKE ADAM M. SANTOS, Teacher I ### Consolidator: - GENOVIE G. TAGUM, Master Teacher II ### Language Editor: - MYRA A. FUENTES, Master Teacher I - ELAINE A. TABOR, Teacher I ### Content Validator: - DUREZA D. DANCAL, Master Teacher I - MYLA JENNIE G. TAN, Master Teacher I - FLORA G. EBCAS, Master Teacher I - GENOVIE G. TAGUM, Master Teacher II - ROWELA G. RUPA, Head Teacher III - MARITES T. TUDIO, Teacher III ## Module 1: Electronic Structure of Matter ### Most Essential Learning Competency: Explain how the Quantum Mechanical Model of the atom describes the energies and positions of the electrons (S9MT-Ila-22). ### What's In - Chain of reactions is happening in our environment, giving rise to various substances, each having a unique property and characteristics, the ionic compounds, covalent compounds, and carbon compounds. Even we are not familiar with them, have been involved in our day-to-day proceedings. They provide support for other processes to materialize. - There is more life, so as there is more to matter. It is hoped that your understanding of the physical world will be deepened as you get through studying all about chemical bonding, a variety of carbon compounds, and the mole under this quarter. - A typical atom consists of three subatomic particles: protons, neutrons, and electrons. Other particles exist as well, such as alpha and beta particles. The Bohr model shows the three basic subatomic particles in a simple manner. Most of an atom’s mass is in the nucleus-a small, dense area at the center of every atom, composed of nucleons. Nucleons include protons and neutrons. All the positive charge of an atom is contained in the nucleus and originates from the protons. Neutrons are neutrally charged. Electrons, which are negatively charged, are located outside of the nucleus. - Bohr’s model accounted for the observed emission spectra of hydrogen and hydrogen-like ions like He+ and Li2+. It did not account, however, for the emission spectra of atoms containing more than one electron. Because of the limitations of Bohr’s model, it was replaced by the Quantum model. In this model, the position of the electrons and their specified energy cannot be measured at the same time. This idea is known as the Heisenberg Uncertainty Principle which states that: It is impossible to know at the same time both the momentum and the position of a particle with certainty. - Though the quantum model tells us that electrons cannot exactly be located in an atom, it can, however, describes the regions where the electrons reside at a given time. The concept of electron density makes it possible that an electron will be found in a particular region of an atom. Denser regions of electron density represent the locations where the electron is most likely to be found, whereas, the regions of less electron density indicate a low probability of finding the electron. The region in space with the greatest probability of finding the electrons in an atom is called an atomic orbital. ### Electron Configuration - The electron configuration of an element describes how electrons are distributed in their atomic orbitals. - Electron configurations of atoms follow a standard notation in which all electron-containing atomic subshells (with the number of electrons they hold written in superscript) are placed in a sequence. For example, the electron configuration of sodium is 1s22s22p63s1. - The order in which electrons are filled in atomic orbitals based on Aufbau principle is illustrated in the mnemonic device. ### Quantum Numbers - To completely describe an electron in an atom, four quantum numbers are needed. These numbers will describe the location and motion of the electrons in an atom. As developed by Niels Bohr, Arnold Sommerfeld and Wolfgang Pauli together with other scientists, these numbers are composed of Principal Quantum number, Angular Momentum Quantum Number, Magnetic Quantum Number and Spin Quantum number. Let´s learn more about these four numbers. - *The Principal Quantum Number (n)* - It is the main energy level or sometimes called shells occupied by the electron of a given atom. It is represented by whole numbers (n=1,2,3,) and having an n value of 1 means the closest to the nucleus, n=2 would be farther and n=3 farther yet. - *Angular Momentum Quantum Number (l)* - It is a number that further divides the shells into subshells. It tells us which subshell is occupied by the electron and its general shape or orbital. The value of l depends on the value of the principal quantum number, n. It can have a positive value of zero to (n-1). So, if n=2, then l could be either 0 or 1. An l=0 represents an s orbital, l=1 for p orbital, l=2 for the d orbital, and l=3 for f orbital. - *Magnetic Quantum Number (ml)* - It is a number that further divides the sub-shells into individual orbitals. It tells us about the orientation in space of a given orbital of a particular energy level (n) and shape (l). There are different possible values for the magnetic quantum number depending on the angular momentum quantum number (l). We can use the following equations: Number of orbitals = 2l+1 Possible values of ml = -l…0…,+l Example If l =2 # of orbitals = 2l+1 = 2(2) +1 = 5 orbitals Values of ml = -2, -1, 0, 1,2 Therefore, if l = 2, the ml has five possible values of -2, -1, 0, 1, 2 which also tell us that the electron has 5 possible orientations in space. - *Spin Quantum Number (ms)* - It tells us about the spin of the electron on its axis. The values are (+1/2) if the electron spins in a clockwise direction and (-1/2) if in a counterclockwise direction. ### Group number, period number valence and core electrons, paired and unpaired electrons - As seen in the periodic table, elements are arranged in a series of vertical columns and horizontal rows. The vertical columns are called family or groups. The elements belonging to the same group have similar properties. The group number in the periodic table represents several valence electrons of the elements in a certain group. For example, all the elements in Group 1 have 1 electron in their outermost shell. - Periods refer to the horizontal rows which are designated as 1,2,3,4,5,6 and 7 in the periodic table. The elements belonging to the same periods have varying properties. All elements in a row have the same number of electron shells. For example, elements Li, Be, B, C, N, O, F, Ne belong to period number 2, they have the same number of electron shells which is two (2). - The electrons of an atom are typically divided into two categories: valence and core electrons. Valence electrons occupy the outermost shell or highest energy level of an atom, while core electrons are occupy the innermost shell or lowest energy levels. This difference greatly influences the role of the two types of electrons in a chemical reaction. Generally, valence electrons can participate in the formation of chemical bonding, but core electrons cannot. While core electrons are not involved in bonding, they influence the chemical reactivity of an atom. For example, the electron configuration of the Oxygen atom is 1s22s22p4, the 1s² electrons in oxygen do not participate in bonding and are called core electrons. The 2s22p4 are valence electrons, which participate in the making and breaking of bonds. - Paired electrons are the electrons in an atom that occur in an orbital as pairs whereas unpaired electrons are the electrons in an atom that occur in an orbital alone. Therefore, paired electrons always occur as a couple of electrons, while unpaired electrons occur as single electrons in the orbital ### What's More - **Activity 1: Subatomic Particles of an Atom** - *Directions:* Identify the subatomic particles being described in each box. Write your answer on the space provided inside the box. - **Activity 2: Predicting the Probable Location of an Electron** - *Directions:* Read and follow the instructions below. 1. Working with any member of your family, draw a dot on the center of the sheet of paper or folder. 2. Draw 5 concentric circles around the dot so that the radius of each circle is 1.0 cm, 3 cm, and 5 cm from the dot. 3. Tape the paper on the floor so that it will not move. 4. Stand on the opposite side of the target from your partner. (Target is the center that represents the nucleus of an atom). Hold a pencil or marker at chest level above the center of the circles you have drawn. 5. Take turns dropping the pencil or marker, to leave 100 dots on the circles drawn on paper or folder. 6. Count the number of dots in each circle and record that number on the data table. 7, Calculate the number of dots per square centimeter (cm2). - **Guide Questions:** - 1. What happens to the number of dots per unit area as the distance of the dots go farther from the center? - 2. Determine the percent probability of finding a dot in each of the circles drawn on the target by multiplying No. of dots /cm² (column E) by the total number of dots (100). - **Activity 3: Electron Configuration** - *A. Directions:* Write the electron configurations of the following elements. 1. Aluminum (13Al) 2. Boron (5B) 3. Copper (29Cu) 4. Magnesium (12Mg) 5. Argon (18Ar) 6. Oxygen (8O) 7. Iodine (53I) 8. Potassium (19K) 9. Calcium (20Ca) 10. Sodium (11Na) - *B. Directions:* Determine what elements are denoted by the following electron configurations. 1. 1s2 2s2 2p6 3s1 2. 1s2 2s2 2p6 3s2 3p 6 4s2 3d10 4p6 5s2 4d6 3. 1s2 2s2 2p6 3s2 3p 6 4s2 3d10 4p6 5s2 4d6 5p6 4. 1s2 2s2 2p4 3s2 3p 6 4s2 4d104p6 5. 1s2 2s2 2p6 3s2 3p6 - **Activity 4: Complete Me!** - *Directions:* Complete the four quantum numbers which describe the location of the highest energy electron of the following atom. ATOM QUANTUM NUMBERS n l m ms 1. H 1 +1/2 2. Li 0 +1/2 3. C 2 -1, 0,1 4. Al 3 +1/2 5. Mg 0 0 - **Activity 5: Group the Period** - *Directions:* Based on the electronic configuration, identify the period number, group number, number of paired electrons, number of unpaired electrons of the following elements. Electron Configuration 1. 11Na - 1s22s22p63s1 2. 35Br - 1s22s22p63s23p64s23d104p5 3. 18Ar - 1s22s22p63s23p6 4. 5B - 1s22s22p1 5. 20Ca - 1s22s22p63s23p64s2 - **What I Have Learned** - *Directions:* Fill in the blanks. Use the word bank to complete the statement. A _______ is the number that is given to a group of elements across the periodic table that have made a round from completing its outer electron shell. The _______ in the periodic table represents number of valence electrons of the elements in a _______ . An _______ or a Lewis pair consists of two electrons that occupy the same molecular orbital but have opposite spins. An _______ is an electron that occupies an orbital of an atom singly, rather than as part of an electron pair. - **What I Can Do** - *Directions:* Discuss briefly the steps on writing an electron configuration of an element. ## Module 2: Ionic and Covalent Compound ### Most Essential Learning Competency: Recognize different types of compounds (ionic or covalent) based on their properties such as melting point, hardness, polarity, and electrical and thermal conductivity. (S9MT-IIb-14) ### What's In - Compounds are defined as substances containing two or more different chemical elements. They have distinct chemical structures characterized by a fixed ratio of atoms held together by chemical bonds. Here, we will discuss two classes of compounds based on the bond type that holds the atoms together: ionic and covalent. ### Types of Compounds 1. Ionic compounds are compounds composed of ions, charged particles that form when an atom (or group of atoms, in the case of polyatomic ions) gains or loses electrons. - A cation is a positively charged ion. - An anion is a negatively charged ion. 2. Covalent or molecular compounds form when elements share electrons in a covalent bond to form molecules. Molecular compounds are electrically neutral. ### Properties of Ionic Compounds - Since the ionic compounds contain ions (cations and anions) which are held together by the strong electrostatic forces of attraction, they show the following general physical properties: - *a. Physical State* ­Ionic compounds are crystalline solids. In the crystal, the ions are arranged in a regular pattern. The ionic compounds are hard and brittle in nature. - *b. Melting and boiling points* Ionic compounds have high melting and boiling points. The melting and boiling points of ionic compounds are high because of the strong electrostatic forces of attraction present between the ions. - *c. Electrical Conductivity* ­Ionic compounds conduct electricity in their molten state and in aqueous solutions. Since ions are free to move in the molten state, they can carry current from one electrode to another in a cell. ### Properties of Covalent Compounds - The covalent compounds consist of molecules that are electrically neutral in nature. The forces of attraction present between the molecules are less strong compared to the forces present in ionic compounds. - Therefore, the properties of the covalent compounds are different from those of the ionic compounds. The characteristic properties of covalent compounds are given below: - *a. Physical State* Because of the weak force of attraction present between discrete molecules, called intermolecular forces, the covalent compounds exist as a gas or a liquid or a solid. For example, O2, N2, CO2 are gases; water and CCl4 are liquids and iodine is a solid. - *b. Melting and boiling points* As the forces of attraction between the molecules are weak in nature, a small amount of energy is sufficient to overcome them. Hence, the melting points and boiling points of covalent compounds are lower than those of ionic compounds. For example, naphthalene’s melting point, which is a covalent compound, is 353K (80°). Similarly, carbon tetrachloride’s boiling point, which is another covalent, liquid compound is 350 K (77°). - *c. Electrical Conductivity* The covalent compounds contain neutral molecules and do not have charged species such as ions or electrons which can carry a charge. Therefore, these compounds do not conduct electricity and are called poor conductors of electricity. ### Natural phenomena that use different physical properties of ionic and covalent compounds 1. The shape of snowflakes results from bonding (and intermolecular) forces in H2O. 2. The lateritic soils are another good example of materials that provide strong interparticle bonds between particles in nature's cyclic wetting and drying processes. 3. The concentration of negative ions is greater in the atmosphere near moving water. Rainstorms, waterfalls, rain showers, rivers and crashing waves are natural negative ion generators. 4. Lightning, the formation of water molecules in these clouds, collide with one another, chipping off electrons and creating an electric charge. 5. A galvanic cell or voltaic cell is an electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell. Electrical current is the movement of charged particles, either electrons or ions, through a conductor. ### What's More - **Activity 1: CLASSIFY ME** - *Directions:* Classify the following properties as either lonic or Covalent compounds. Write ionic or covalent on the space before each property. 1. Atoms share electrons to become stable. 2. High melting and boiling points 3. Conduct electricity when melted 4. Usually occurs between non-metals 5. Poor electrical conductors in all phases 6. Many soluble in non-polar liquids but not in water 7. Crystalline solids (made of ions) 8. Metal atoms give electrons while non-metal atoms get electrons to become stable 9. Usually occurs between metals and non-metals 10. Hydrogen and another non-metal chemically combines through covalent bonding. 11. Low melting and boiling points 12. Many soluble in water but not in non-polar liquid - **Activity 2: MATERIAL THING** - *Directions:* Based on the properties of the following materials, determine whether they are made of primarily ionic compounds or covalent compounds: a) telephone receiver: b) concrete: c) gasoline: d) candy corn: - **Activity 3: Ionic vs. Covalent** - *Directions:* Determine if the elements in the following compounds are metals or non-metal. Then, identify the type of compound as to ionic or covalent. Element 1 Element 2 lonic or Covalent Compounds CCI4 (metal or non-metal) (metal or non-metal) NaCl SO2 CaO HF K2O Fe2O3 O2 CuCl2 AIF3 - **Activity 4: BANKING TERMS** - *Directions:* Use the word bank to fill in the blanks below (some words can be used more than once). Word Bank ionic neutral covalent metal cation nonmetal anion two bonding compound 1.Atoms become stable by _______ and forming _______. 2.All compounds are _______. 3.A stable binary compound is formed when _______ and _______ elements bond. 4.lonic compounds are formed between _______ and _______. 5.Covalent compounds are formed between two _______. 6.In a/an _______ bond, valence electrons are shared to form a stable _______ binary compound. 7.In a/an _______ bond, electrons are transferred to form a stable _______ binary compound. 8. The names of _______ compounds contain prefixes that indicate the number of atoms of each element present. 9. A/an _______ is a positively charged ion. 10.A/an _______ is a negatively charged ion. - **What I Have Learned** - *Directions:* Write TRUE if the statement is correct, and if false, change the underlined word/s to make the statement correct. 1. The ionic compounds are hard and brittle in nature. 2. Covalent or molecular compounds form when elements transfer electrons in a covalent bond to form molecules. 3. A cation is a positively charged ion. 4. Covalent compounds have high melting and boiling points. 5. Ionic compounds are compounds composed of ions, charged particles that form when an atom (or group of atoms, in the case of polyatomic ions) gains or loses electrons. - **What I Can Do** - *Directions:* List three differences between ionic and covalent compounds. 1. 2. 3. ## Module 3: Electronic Structure of Matter ### Most Essential Learning Competency: Explain how ions are formed (S9MT-Ile-f-16) ### What's In - Tiny atoms are what comprise everything in this world. The varieties of material we are enjoying right now are products of the unending chemical reactions and combination of different atoms. Going through this lesson will make you understand what is happening in the atoms during the formation of compounds, and to determine whether the atoms transfer or share electrons to become stable. - Why do ions form? All elements want to be like their closest noble gases and have 8 electrons in their last energy level. Some elements have to lose electron/s while other gain electron/s to get this "stable state." - In the formation of an ionic bond, atoms loss or gain valence electron/s to complete their outer shell and attain a noble gas configuration. Atoms that gained or lose electrons to have eight valence electrons in their outer shell follow the octet rule or the rule of eight valence electrons. This tendency of atoms to loss or gain electrons is called electronegativity. Electronegativity ranges from 0.1(lowest) to 4.0 (highest). ### Formation of Ions based on Electronegativity - Ion (charged particle) can be produced when an atom gains or loses one or more electrons. - *Cation (positive + ion)* – is formed when a neutral atom gains an electron - *Anion (negative - ion)* - is formed when a neutral atom gains an electron - To write an element's Lewis Electron Dot Symbol (LEDs), we place dots representing its valence electrons, one at a time, around the element's chemical symbol. Up to two dots are placed above, below, to the left, and to the right of the symbol (in any order, as long as elements with four or fewer valence electrons have no more than one dot in each position). The next dots, for elements with more than four valence electrons, are again distributed one at a time, each paired with one of the first four. ### What's More - **Activity 1: Bonding by Transfer of Electrons** - *Directions:* Read and follow the procedure below. 1. Select a metallic and non-metallic element. Write the Lewis Symbol of the selected elements. Take note of the electronegativity value of both elements. Subtract the electronegativity value of the metallic element from the non-metallic element Na. EN = 0.90 Thus: CI: EN = 3.0 1.0-0.90 = 2.1 *If the difference is greater than 1.9, complete transfer of electron/s is possible* 2. With the use of an arrow, show the complete transfer of electrons Na EN = 0.90 :CI: EN = 3.0 3. Indicate the formation of cation and anion Na+CI- 4. Make 5 combinations that will result to ionic bonding by following steps 1-3 - *Guide Questions:* 1. What kind of element forms cation after ionic bonding? 2. What kind of element forms anion after ionic bonding? 3. Why do ions form after ionic bonding? 4. Did the atoms attain stability after ionic bonding? Explain your answer. 5. How can you tell that ionic bonding will take place between metals and non-metals? 6. Will all combination of metals and non-metals form ionic bond? Why? Why not? - **Activity 2: Add mi lons!** - *Directions:* Complete the table by supplying the needed information. # Valence #Electrons # Electrons Element Electrons to gain to use lons Formed/Name Li 1 0 1 Li +1 / cation N 5 3 0 N -3 / anion Ο Ca Br S CI K Mg Be - **Activity 3: Who Am I: Cation or Anion?** - *Directions:* Classify the elements as to cations or anions. Refer to the electronegativity values indicated in the element symbol (cation if the number is below 2 and anion if it it is higher than 2). Write the symbol of the elements in the table. Cation Anion C 2.5 Mn 1.5 Tc Cs 1.9 0.7 Ag 1.9 S 2.5 Zr 1.4 P 2.1 1 2.5 d 3.0 Zn 1.6 - *Guide Questions:* 1. What kind of elements are cations? 2. What kind of elements are anions? - **Activity 4: Gain or Lose: Its lons!** - *Directions:* Complete the table by supplying the needed information. Symbol Name of the Electronegativity Low or high lons formed element values electronegativity (cation or anion) 1. Mg 2. Sc 3. Ο 4. F 5. P 6. Cu 7. Fe 8. Br 9. Se 10. N - *Questions:* 1. What are elements that are cations? anions? Cations Anions 2. How did you differentiate cations and anions based on their tendency to loss or gain electrons? - **Activity 5: Every Dot Counts** - *Directions:* Complete the table. Element Electron Valence Electron Lewis Ion Formed configuration Electron Gain Loss Symbol /type Ex 1. Lithium (Li) [He]2s1 1 0 1 Li Li + Cation Ex 2. Oxygen (O) [He]2s22p4 6 2 0 :. O2- Anion 1. Beryllium 2. Boron 3. Barium 4. Nitrogen 5. Chlorine 6. Fluorine 7. Sulfur 8. Magnesium 9. Potasium 10. Sodium - *Guide Questions:* 1. What is Lewis Electron Dot Symbol (LEDS)? 2. How are ions formed? 3. Why is Lewis Electron Dot Symbol (LEDS) important in showing the formation of ions? ## Module 4: The Carbon Atom ### Most Essential Learning Competency: Explain how the structure of carbon atom affects the type of bonds it forms (S9MT-IIg-17) ### What's In - Carbon (C), a nonmetallic chemical element in Group 14 (IVA) of the periodic table. Although widely distributed in nature, carbon is not particularly plentiful-it makes up only about 0.025 percent of the Earth's crust yet it forms more compounds than all the other elements combined. Carbon atoms have four electrons in their valence shell, and that the octet rule dictates that atoms tend to react in such a way as to complete their valence shell with eight electrons. Carbon atoms do not complete their valence shells by donating or accepting four electrons. Instead, they readily share electrons via covalent bonds. Commonly, carbon atoms share with other carbon atoms, often forming a long carbon chain referred to as a carbon skeleton. When they do share, however, they do not share all their electrons exclusively with each other. Rather, carbon atoms tend to share electrons with a variety of other elements, one of which is always hydrogen. Carbon and hydrogen groupings are called hydrocarbons. Carbon's affinity for covalent bonding means that many distinct and relatively stable organic molecules nevertheless readily form larger, more complex molecules. It can form single, double, or triple bonds with other elements. - Carbon atoms may contain different numbers of neutrons forming isotopes. Isotopes of carbon are Carbon 13 and 14. ### What's More - **Activity 1: CARBO-KNOWS** - *Directions:* Create an element square for Carbon using the given information on the left. Follow the format given for Iron (Fe). - CARBON (from the Latin word "carbo" means "coal") is an element with a chemical symbol of C, an atomic number of 6 and atomic mass of 12.011. Each carbon atom has 6 electrons-two located in the inner orbit while the remaining 4 are valence electrons. It also has 6 protons and neutrons inside the nucleus. - **Activity 2: ATOMIC MODEL** - *Directions:* From the information given in Activity 1, draw the atomic model of a carbon atom by completing the orbitals using the symbols for protons, electrons, and neutrons. - *Symbols:* electrons protons neutrons - **Activity 3: Organic vs. Inorganic** - *Directions:* With the given the chemical formula, identify the type of substances by writing ORGANIC or INORGANIC on the space provided before the number. 1. Glucose -C6H1206 2. Hydrogen Peroxide- H2O2 3. Isopropyl alcohol -C2H5OH 4. Baking Soda - NaHCO3 5. Penicillin- C16H18N2O4S 6. Sand- SiO2 7. Caffeine- C8H10N4O2 8. Table salt- NaCl 9. Acetone- C3H6O 10. Water - H2O - **Activity 4: Getting to Know You** - *Directions:* Fill in the table with the properties of some organic substances. Materials 1. Kerosene Color Odor (strong or weak) Phase (solid, liquid or gas) Volatility (volatile, nonvolatile) Flammability (flammable, non-flammable) Yellow strong liquid nonvolatile flammable 2. Baby Oil 3. Diesel Oil 4. Ethyl Alcohol 5. Isopropyl Alcohol 6. Vegetable Oil - *Guide Questions:* - 1. Are all materials liquid? - 2. Which material/s have strong odor? - 3. Which material/s have weak odor? - 4. Are they all colorless? - 5. Which material/s is/are flammable? - 6. Which materials are volatile? - 7. Why is it important to know the different properties of an organic and inorganic material? - **What I Have Learned** - *Directions:* Write TRUE if the statement is correct and if false, change the underlined word/s to make the statement correct. 1. Carbon is a nonmetallic element that has an atomic number of 6. 2. Carbon-13 is an isotope of carbon with 14 neutrons. 3. Alkanes are formed when single bonds are formed by a carbon atom with another carbon or atoms of other elements. 4. The atomic number of carbon is 6, which means that there are 6 electrons and 6 neutrons in a carbon atom. 5. Organic compounds always contain carbon and oxygen. 6. Carbon atoms always tend to share electrons forming a covalent bond. 7. Most organic compounds are soluble in water. 8. Water (H2O) is an organic compound. 9. Inorganic compounds are more electrically conductive compared to organic compounds 10. Organic compounds are typically less dense than inorganic compounds. - **What I Can Do** - *Directions:* Look around your house and list down 5 organic and 5 inorganic substances/materials. Cite their uses. ORGANIC MATERIALS Uses 1 2 3 4 5 INORGANIC MATERIALS 1 2 3 4 5