Year 9 Chemistry Booklet 2023 PDF

NAME: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ Year 9 Chemistry **Calculators are allowed for this topic test. A periodic table will be provided (you cannot bring in your own).** **[Some Year 8 Chemistry Revision]** - **Types of substances:** - **Elements vs Compou...

NAME: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ Year 9 Chemistry **Calculators are allowed for this topic test. A periodic table will be provided (you cannot bring in your own).** **[Some Year 8 Chemistry Revision]** - **Types of substances:** - **Elements vs Compounds** - **Atoms vs Molecules vs Lattices** - **What is a chemical formula?** - **Metals vs Non-Metals** - **Characteristics of metals** - **Characteristics of non-metals.** **[Part 1: Atomic Structure & The Periodic Table]** - **3 subatomic particles in atoms** - **Relative masses** - **Charges** - **Location in atom (Nucleus or Shells)** - **Using the periodic table** - **Finding out No. of Protons, Neutrons, Electrons** - **What is an atomic symbol? Why do some use weird letters?** - **Where are the Metals vs Non-Metals (& Metalloids)** - **Groups vs Periods** - **Isotopes** - **How to write isotope names** - **Stable vs Unstable** - **Ions** **[Part 2: Electron Shell Configuration]** - **Capacity of each shell.** - **Valence Electrons & Valence Shell** - **How to write out an electron configuration** - **Using the periodic table** - **How to find out the no. of valence electrons** **[Part 3: Ionic Bonding]** a. **Finding out an ion's charge** - **Difference between an atom and an ion** - **Cation vs Anion** - **How to write the chemical formula for an ion** - **Getting full valence shell** - **When will an atom lose or gain electrons?** - **What will an ion's charge be?** - **Using the Periodic table** - **How to find out the no. electrons lost or gained?** - **How to find out the charge? Cation or Anion?** b. **Ionic Compounds** - **Which elements will form ionic bonds?** - **Identify a covalent bond from its chemical formula** - **How does an ionic bond work?** - **How to work out the formula of an ionic compound** - **E.g. Na & Cl , Ca & Cl** - **Short-cut method -- Crossover rule** - **How to name an ionic compound** - **How to draw a diagram of an ionic bond** **[Part 4: Covalent Bonding]** - **Which elements will form covalent bonds?** - **Identify a covalent bond from its chemical formula** - **How does a covalent bond work?** - **Difference between ionic bonds and covalent bonds** - **How to draw a diagram of a covalent bond** - **Dot and Cross Diagrams** - **Lewis Diagram (e.g. Cl** ─ Cl , O = O) - **How to work out the formula of a covalent molecule through diagrams** **[Part 4.5: Polyatomic Ions]** - **What is a polyatomic ion?** - **Why does Hydroxide (OH^-^) have a charge?** - **Be able to recognise chemical formula that involve polyatomic ions** - **E.g. NaOH, Na~2~CO~3~, Mg(OH)~2~** - **Be able to work backwards and identify a polyatomic ion's charge by determining the charge of the metal it's bonded to.** **[Part 5: Metallic Bonding]** - **What is metallic bonding?** - **Why does metallic bonding occur?** - **What are delocalised electrons?** - **How does this influence the properties of a metal?** - **Conducts electricity** - **Malleable and Ductile** **[Part 6: Groups and Trends in the Periodic Table]** - 4 notable groups in the Periodic Table - Alkali Metals - Alkali Earth Metals - Halogens - Nobel Gasses - Which groups are most reactive? Why? - Which group doesn't react? Why?**\ ** **Year 8 Chem Revision** **[Elements, Compounds and Chemical Formula ]** **3. Using the periodic table, what is the atomic symbol for:** **a) Oxygen? b) Hydrogen? c) Neon?** **4. a) Beneath each of these images, write either "Element" or "Compound"** **b) Beneath each of these images, write either "Single Atom" or "Molecule" or "Lattice"**  **5. The chemical formulas for the substances above are O~2~, Ne, H~2~O and NaCl. Write the correct chemical formula next to the correct diagram of the substance.** **6. What would be the chemical formula for each of the three following substances?** **\ ** **Year 8 Chem Revision** **8. Mabel and Marco writes the chemical formula for the following as such:** **Explain why their formulas are not written correctly.** **9. a) What would be the chemical formula for each of the two following substances?**  b\) What do you think is the principle when it comes to chemical formula for lattices like those above? **Year 8 Chem Revision** **[Metals, Non-Metals & Metalloids]** **11.** Fill in the labels above and the questions below [Non-metals] are found on the \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ of the periodic table. Properties: [Metalloids:] Properties: [Metals] are found on the \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ of the periodic table. Properties: **[\ ]** **Part 1: Atomic Structure & The Periodic Table** **[Atomic Structure]** Elements are made up of many atoms that are the same. An atom is made up of **protons, neutrons** and **electrons**. The **nucleus** of an atom is made up of protons and neutrons and the electrons orbit around the nucleus in what is called an **electron shell**.  **...........................** are negatively charged (-) **...........................** are positively charged (+)........................... have no charge (0) An atom has an overall \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ **charge**, because it has an equal amount of \_\_\_\_\_\_\_\_\_\_ and \_\_\_\_\_\_\_\_\_. The \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ in an atom determines an elements chemical behaviour because they are the most outer part of an atom. \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ have a relative mass of 1. \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ have a relative mass of 1. \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ are so small that their relative mass is negligible. The **atomic mass** is therefore determined by the sum of particles inside the \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_. **Part 1: Atomic Structure & The Periodic Table** **[Periodic Table]** The Periodic Table gives information about the structure of an atom. +-----------------------------------------------------------------------+ | ** 6** | | | | **C** | | | | **Carbon** | | | | 12.011 | +-----------------------------------------------------------------------+ **ATOMIC MASS NUMBER:** The total number of \_\_\_\_\_\_\_\_\_\_\_\_ and \_\_\_\_\_\_\_\_\_\_\_\_ in an atom. **ATOMIC NUMBER:** The total number of \_\_\_\_\_\_\_\_\_\_\_\_\_\_. Since atoms are neutral, the number of protons and electrons must equal each other. Sometimes, a periodic table may change the formatting. Regardless, - the smaller number will always be the atomic number, - and the bigger number will always be the atomic mass. **Part 1: Atomic Structure & The Periodic Table** **Q.** Work out the following from this information: **Q.** Why do some elements have symbols with letters that don't match up to their names? **[Isotopes]** An isotope is a *variation* of an atom.\ Different isotopes have the same number of **protons**, but different number of **neutrons**. Some Isotopes are **unstable**, meaning their nucleuses decay and break down easily. They are radioactive. An isotope is written like this: **\[Element Name\] - \[Atomic Mass\] e.g. Carbon-12** **Q.** Write the names of the following isotopes. (You will need to use a periodic table). **a.** A Carbon Atom with 7 Neutrons: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ **b.** An Iron Atom with 31 Neutrons: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ **c.** A Gold Atom with 121 Neutrons: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ **Q.** List how many Neutrons there are in the following Isotopes: a. Carbon-14 \_\_\_\_\_\_\_\_\_ b. Iron-54:\_\_\_\_\_\_\_\_\_ c. Gold-170:\_\_\_\_\_\_\_\_ **Q.** With reference to isotopes, explain why the atomic mass of an atom on the periodic table is usually not a whole number: **Part 1: Atomic Structure & The Periodic Table** **[Ions]** An ion is what we call an atom when it has a charge. For an atom to have a charge, it must have an uneven amount of electrons (-) to protons (+). It therefore must have gained or lost \_\_\_\_\_\_\_\_\_\_\_\_\_\_. Fill in the questions below:  **\ ** **Part 1: Atomic Structure & The Periodic Table** **\ Atoms, Ions & Isotopes. What does it all mean?** 1. Neutrons in the nucleus make the atom \_\_\_\_\_\_\_\_\_\_\_\_\_\_ but do not affect the **chemical** properties of the element. 2. When an atom has extra **neutrons** we call it an \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_. 3. Some atoms with extra neutrons are \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_. They emit \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ from their nucleus to reach a more stable state. We say these atoms are \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_. Ions are something completely different! 4. Ions are formed when an atom loses or gains \_\_\_\_\_\_\_\_\_\_ 5. The positive ions are called \_\_\_\_\_\_\_\_\_\_\_\_ and are formed by \_\_\_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_\_\_\_ 6. The negative ions are called\_\_\_\_\_\_\_\_ and are formed by \_\_\_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_\_\_\_ 7. An Ion's chemical symbol should show it's \_\_\_\_\_\_\_\_\_\_\_ e.g., Mg^2+^ **In Summary:** **\ ** **Part 2: Electron Shell Configuration** A diagram of a periodic table Description automatically generated **Part 2: Electron Shell Configuration** **[Electron Shells]** **RULE FOR ELECTRON SHELLS** **Shell 1: 2** **Shell 2: 8** **Shell 3: 8** **Shell 4: 18**  [Example]\ A neutral carbon atom has 6 protons and 6 electrons.\ The **electron shell diagram** will look like this *Remember:* Electrons occupy the inner shells first, then spill over. 1. Practice drawing the electron shell diagrams of the following elements: **Part 2: Electron Shell Configuration** ELECTRON SHELL DIAGRAM PRACTICE: Draw **diagrams** for the following atoms and state their **electronic configuration.** Boron Fluorine Chlorine Lithium Aluminium Hydrogen **[\ ]** **Part 2: Electron Shell Configuration** **[Electron Dot Diagrams (easy version)]** Electron dot diagrams are a convenient (and easier) way of representing what is happening in an atom. They show us how many **\...\...\...\...\...\...\...\...\...\...\...\...\...\...\...\...\...** an atom has. ***Valence electrons refer to the electrons in the outer most shell of an atom.*** **Example** Diagram of a CARBON atom. Electron dot diagram of CARBON  *(Only show valence electrons)* Electron dot diagrams show us **[the number of electrons in the outer shell of an atom]**. Each dot represents one electron. [Draw electron dot diagrams for the following:] (Some have already been done for you) **Part 2: Electron Shell Configuration** **[Using the periodic table]** **The periods in a periodic table are arranged as per electron shell capacity.** **E.g. the first period has 2 atoms, because these atoms only fill their first shell of 2. The second period has 8 atoms, because these atoms start and finish filling up their second shell of 8. And so on.** **So looking at the periodic table, we can see that the shell capacities are; 2, 8, 8, 18, 18, 32, 32.**  **How do we know the last 2 periods have 32 atoms in them? Well the "Lanthanides" and "Actinides" are a collection of atoms that are meant to be in the 6^th^ and 7^th^ periods, but are never usually depicted this way because there isn't usually enough space.** **Really, the periodic table is supposed to look like this:** **Fill in the blanks:** **All atoms in the same \_\_\_\_\_\_\_\_\_\_ have the same number of electrons in the outermost shell (\_\_\_\_\_\_\_\_\_\_\_\_\_ electrons).** **All atoms in the same \_\_\_\_\_\_\_\_\_\_ have the same number of occupied \_\_\_\_\_\_\_\_\_\_\_\_\_ [\ ]** **Part 3: Ionic Bonding -- Finding out an Ion's Charge** **[Forming Ions]** Diagram Description automatically generated Atoms want to get **[full outer shells].** When ionically bonding, they will either **lose electrons** or **gain electrons.** (Whichever is easiest). **Q.** Which of the following is the correct ion for Oxygen? Diagram, schematic Description automatically generated ***Oxygen Atom*** **Q**. What will Oxygen's charge be when it becomes an ion? (Just like Sodium above, you work this out by counting the number of protons (+) to electrons (-). Oxygen's Charge: \_\_\_\_\_\_\_\_\_\_\_\_ **Part 3: Ionic Bonding -- Finding out an Ion's Charge** **[Now draw the following ]** (This time, you don't need to draw all the protons and neutrons. You can just draw a nucleus and label the number of protons and neutrons like in the diagrams above) Magnesium **Atom** Is it easier for Magnesium to gain or lose electrons? Magnesium **ion** Count up the number of protons to electrons, and now write down Magnesium's **charge**. -------------------- ------------------------------------------------------- ------------------- ----------------------------------------------------------------------------------------- Chlorine **Atom** Is it easier for Chlorine to gain or lose electrons? Chlorine **ion** Count up the number of protons to electrons, and now write down Magnesium's **charge**. 1\. Write the symbol for each of the following atoms and for the ion they form. (Sodium is done for you) **Sodium** **Nitrogen** **Potassium** **Fluorine** **Helium** **Chlorine** **Sulphur** ---------- ------------ -------------- --------------- -------------- ------------ -------------- ------------- **Atom** Na **Ion** Na^+^ 2\. How many electrons have been lost or gained by the following ions? a. Pb^4+^ \_\_\_\_\_\_\_\_ c) Cr^3+^ \_\_\_\_\_\_\_\_\_ e)H^+^ \_\_\_\_\_\_\_\_\_\_\_ b. **Part 3: Ionic Bonding -- Finding out an Ion's Charge** **[Using the Periodic Table to identify Ionic Charges]** Group 1 elements all wish to **lose** \_\_\_ electron, and therefore form ions with a charge of \_\_\_\_ Group 2 elements all wish to **lose** \_\_\_ electrons, and therefore form ions with a charge of \_\_\_\_ Group 3 elements all wish to **lose** \_\_\_ electrons, and therefore form ions with a charge of \_\_\_\_ Group 4 elements can either lose or gain \_\_\_ electrons, however they do not normally form ions. (explained later) Group 5 elements all wish to **gain** \_\_\_ electrons, and therefore form ions with a charge of \_\_\_\_ Group 6 elements all wish to **gain** \_\_\_ electrons, and therefore form ions with a charge of \_\_\_\_ Group 7 elements all wish to **gain** \_\_\_ electrons, and therefore form ions with a charge of \_\_\_\_ Group 8 elements already have a full outer shell of electrons, and therefore do not form ions. **Circle the correct terms:** **Part 3: Ionic Bonding -- Ionic Compounds** **[Cations vs Anions]** Atoms that **[gain electrons have a negative charge]** because they now have more electrons, which are negatively charged. These are called.................................. Atoms that **[lose electrons have a positive charge]** because they now have more protons, which are positively charged. They are called...................................... Which of these are Cations and which are Anions? a. Pb^4+^ \_\_\_\_\_\_\_\_ c) Cr^3+^ \_\_\_\_\_\_\_\_\_ e)H^+^ \_\_\_\_\_\_\_\_\_\_\_ b. **[Putting it all together (QUICK REVIEW)]** Identify the number of **protons** and **neutrons** for each of the following elements (round atomic mass to nearest whole number): Beryllium Oxygen Aluminium ----------- ------------ ----------- Sodium Phosphorus Argon Write the electronic configuration for each of the following **atoms**: Beryllium Oxygen Aluminium ----------- ------------ ----------- Sodium Phosphorus Argon Write the electronic configuration for each of the following **ions**: Be^2+^ O^2-^ Al^3+^ -------- ------- ---------------------- Na^+^ P^3-^ Ar -- no ions formed Draw the electron shell diagram for each of the following **atoms**: ----------- -------- ----------- Beryllium Oxygen Aluminium ----------- -------- ----------- Draw the electron shell diagram from each of the following **ions**: -------- ------- -------- Be^2+^ O^2-^ Al^3+^ -------- ------- -------- **[\ ]** **Part 3: Ionic Bonding -- Ionic Compounds** **[\ Ionic Bonds]** Ionic bonding is a type of chemical bonding that takes place between a metal and a non-metal 1. The metal gives away electrons to the non-metal, who receives the electrons 2. The metal becomes a positive ion (cation) 3. The non-metal becomes a negative ion (anion) 4. Positive ion and negative ion attract, forming an ionic bond. Ionic Bonds and Ionic Compounds \| CK-12 Foundation **So how do you know which atoms will lose electrons and which atoms gain electrons?** **If the outer shell contains LESS THAN FOUR electrons it will........................... those electrons.** **If the outer shell contains GREATER THAN FOUR electrons it will................. electrons from another atom.** On the following page, **draw diagrams of ionic bonds** like the one above with Sodium and Fluorine to show how each of the following compounds are formed.  Sometimes you need more than one of each type of atom to make sure they all get full outer shells. E.g. **Calcium Chloride** **to the right**. Calcium must give away 2 electrons, chlorine must receive 1. Therefore 1 calcium will give each electron to 2 separate Chlorine atoms, becoming CaCl~2~. **Part 3: Ionic Bonding -- Ionic Compounds** +-----------------------------------------------------------------------+ | **Lithium chloride** | | | | Chemical Formula: | +=======================================================================+ | **Magnesium fluoride** | | | | Chemical Formula: | +-----------------------------------------------------------------------+ | **Aluminium sulfide** | | | | Chemical Formula: | +-----------------------------------------------------------------------+ | **Calcium oxide** | | | | Chemical Formula: | +-----------------------------------------------------------------------+ **Part 3: Ionic Bonding -- Ionic Compounds** **[Additional Practice Questions]** Deduce the **name** and **chemical formula** if the following elements were to react to form ionic compounds. Refer to your periodic table and follow the steps outlined below. **Example: Aluminium and Chlorine** Step 1 -- how many valence electrons? Al Cl ------------------ ------------------ **3 valence e-** **7 valence e-** Step 2 -- who needs to **lose** electrons and how many? Who needs to **gain** electrons and how many? Al Cl --------------- --------------- 3 valence e- 7 valence e- **Lose 3 e-** **Gain 1 e-** **Al^3+^** **Cl^-^** Step 3 -- in what **ratio** will these elements react? +-----------------------------------+-----------------------------------+ | **Calcium + Bromine** | **Lithium + Iodine** | | | | | Chemical formula: | Chemical formula: | | | | | Name: | Name: | +===================================+===================================+ | **Sodium + Nitrogen** | **Potassium + Chlorine** | | | | | Chemical formula: | Chemical formula: | | | | | Name: | Name: | +-----------------------------------+-----------------------------------+ **Part 3: Ionic Bonding -- Ionic Compounds** +-----------------------------------+-----------------------------------+ | **Beryllium + Fluorine** | **Lithium + Oxygen** | | | | | Chemical formula: | Chemical formula: | | | | | Name: | Name: | +===================================+===================================+ | **Aluminium + Oxygen** | **Magnesium + Bromine** | | | | | Chemical formula: | Chemical formula: | | | | | Name: | Name: | +-----------------------------------+-----------------------------------+ | **Calcium + Sulphur** | **Magnesium + Nitrogen** | | | | | Chemical formula: | Chemical formula: | | | | | Name: | Name: | +-----------------------------------+-----------------------------------+ **Part 3: Ionic Bonding -- Ionic Compounds** **[Chemical formulas]** Sodium chloride, made from sodium ions (Na^+^) and chloride ions (Cl^-^), has the chemical formula NaCl. Note: the total charge of the cations and anions in the crystal lattice adds to zero. Eg: magnesium chloride is MgCl~2~. The magnesium ion (Mg^2+^) has a charge +2 and the chloride ion (Cl^-^) has a charge -1, so each magnesium ion needs two chloride ions to balance the total charge. Similarly, sodium nitride is Na~3~N. The sodium ion (Na^+^) has a charge of +1 and the nitride ion (N^3-^) has a charge of -3, so there must be three sodium ions to balance the charge of each nitride ion in the crystal lattice. **[In Aluminium Oxide:]** Aluminium Ions have a charge of 3+. Oxide ions have a charge of 2-. Aluminium must **\[** gain / lose **\]** \_\_\_\_\_\_\_ elections. While Oxygen must **\[** gain / lose **\]** \_\_\_\_\_\_\_ elections. We need \_\_\_\_\_\_\_ aluminium and \_\_\_\_\_\_\_\_ oxygens. Chemical Formula: \_\_\_\_\_\_\_\_\_\_\_\_\_ ***[Short-Cut to working out the chemical formula:]***  **Step 1:** Write the ions with their charges: Fe^3+^ O^2-^ **Step 2:** Swap and drop the numbers ONLY (do not drop the +/- signs!) This is the formula for iron oxide. All charges are balanced when 2 Fe^3+^ ions combine with 3 O^2-^ ions. **Part 3: Ionic Bonding -- Ionic Compounds** Element 1+ 2+ 3+ 4+ --------- ------------ -------- ---------------- -------- ----------------- -------- ---------------- -------- **Cu** Copper (I) Cu^1+^ Copper (II) Cu^2+^ \- \- \- \- **Co** \- \- Cobalt (II) Co^2+^ Cobalt (III) Co^3+^ \- \- **Fe** \- \- Iron (II) Fe^2+^ Iron (III) Fe^3+^ \- \- **Mn** \- \- Manganese (II) Mn^2+^ Manganese (III) Mn^3+^ Manganese (IV) Mn^4+^ 1. **Determine** the chemical names of the following ionic compounds from their chemical formulas. Chemical formula Chemical name ------- ------------------ --------------- **a** NaCl **b** PbI~2~ **c** BaS **d** Li~3~N **e** Al~2~O~3~ **f** K~3~P **g** CaS **j** NaBr **k** CaO **m** CuBr **o** KI **p** CuO **r** NaI **Part 3: Ionic Bonding -- Ionic Compounds** **MORE PRACTICE:** Cation Anion Chemical name Chemical formula ------- ------------------------------------------------------------------------- ------- --------------- ------------------ **a** Na^+^ O^2-^ **b** Mg^2+^ Cl^-^ **c** Zn^2+^ S^2-^ **d** Al^3+^ P^3-^ **e** Al^3+^ C^4-^ BELOW ARE HARDER (Remember to use Roman Numerals for Transition Metals) **f** Cu^2+^ S^2-^ **g** Mn^4+^ O^2-^ **h** Cr^6+^ Cl^-^ **i** Fe^2+^ S^2-^ **j** Fe^3+^ S^2-^ 2. **Determine** the cations, anions, chemical name and formula of the ionic compounds made from the following elements. (Use the periodic table to determine the element's charges when they are ions). Element 1 Element 2 Cation Anion Chemical name Chemical formula ------- ----------- ----------- -------- ------- --------------- ------------------ **a** Be P **b** Ga N **c** Al F **d** Ca Cl **e** Ga Br **f** Al P **g** Na P **h** Mg Se **Part 4: Covalent Bonding** **[Covalent Bonding]** Covalent bonding is a type of chemical bonding that takes place between two [non-metals] 1. Non-metals usually have \>4 valence electrons, so both are unwilling to give away electrons 2. Instead, they '**share**' a pair of electrons, forming a covalent bond. 3. No electrons leave their original atoms, so the atoms **remain neutral** (no ions are formed)   **Part 4: Covalent Bonding** **[How to work out the structure of a covalent molecule]** There are 3 simple steps. You need to use the Lewis Dot Diagram to help you find out. *E.g. "Draw an Electron Dot Diagram Structure for PF~3~"**[\ ]*** **Part 4: Covalent Bonding** +-----------------------+-----------------------+-----------------------+ | **[Molecule]{.underli | **[Structures]{.under | | | ne}** | line}** | | +=======================+=======================+=======================+ | H~2~ | Electron Dot Diagram | Electron Dot Diagram | | | (Working Out Space) | | | | | | | |  | | +-----------------------+-----------------------+-----------------------+ | | Dot and Cross Diagram | Structural Diagram | | | | | | |  | | +-----------------------+-----------------------+-----------------------+ | Cl~2~ | Electron Dot Diagram | Electron Dot Diagram | | | (Working Out Space) | | +-----------------------+-----------------------+-----------------------+ | | Dot and Cross Diagram | Structural Diagram | +-----------------------+-----------------------+-----------------------+ | HCl | Electron Dot Diagram | Electron Dot Diagram | | | (Working Out Space) | | +-----------------------+-----------------------+-----------------------+ | | Dot and Cross Diagram | Structural Diagram | +-----------------------+-----------------------+-----------------------+ | H~2~O | Electron Dot Diagram | Electron Dot Diagram | | | (Working Out Space) | | +-----------------------+-----------------------+-----------------------+ | | Dot and Cross Diagram | Structural Diagram | +-----------------------+-----------------------+-----------------------+ **Part 4: Covalent Bonding** **[Molecule]** **[Structures]** ---------------------------- ------------------------------------------ ---------------------- CO~2~ Electron Dot Diagram (Working Out Space) Electron Dot Diagram Dot and Cross Diagram Structural Diagram NH~3~ Electron Dot Diagram (Working Out Space) Electron Dot Diagram Dot and Cross Diagram Structural Diagram CH~4~ Electron Dot Diagram (Working Out Space) Electron Dot Diagram Dot and Cross Diagram Structural Diagram N~2~ Electron Dot Diagram (Working Out Space) Electron Dot Diagram Dot and Cross Diagram Structural Diagram **Part 4: Covalent Bonding** ---------------------------------------------------------------------------------------------- **[Molecule]** **[Structures]** ---------------------------- ------------------------------------------ ---------------------- CS~2~ Electron Dot Diagram (Working Out Space) Electron Dot Diagram Dot and Cross Diagram Structural Diagram C~2~H~6~ Electron Dot Diagram (Working Out Space) Electron Dot Diagram Dot and Cross Diagram Structural Diagram C~2~H~4~\ Electron Dot Diagram (Working Out Space) Electron Dot Diagram *(Challenge)* Dot and Cross Diagram Structural Diagram ---------------------------------------------------------------------------------------------- **[\ ]** **Part 4: Covalent Bonding** **[Determining Chemical Formula of Covalent Compounds]** 1. For these ones, you will need to work backwards! **Elements** **Atoms** **Molecule** **Chemical Formula** --------------------- ----------- -------------- ---------------------- Hydrogen & Fluorine Carbon & Fluorine Hydrogen & Bromine Hydrogen & Sulphur **[Ionic vs Covalent]** 2. Draw diagrams illustrating the difference between ionic bonds and covalent bonds. **Part 4: Covalent Bonding**  6\. Describe three differences between ionic bonds and covalent bonds. ------------------------------- ---------------------------------- **[Ionic Bonds]** **[Covalent Bonds]** ------------------------------- ---------------------------------- **Part 4.5: Polyatomic Ions EXTENSION** **[Polyatomic Ions]** Sometimes you might see a *polyatomic ion*. This is a **group of atoms that are covalently bonded**, but have also **taken some electrons using an ionic bond**. A polyatomic ion is almost always going to be an anion (negatively charged ion). **Example 1: Hydroxide (OH^-^) is a polyatomic ion** Diagram Description automatically generated **Example 2: Carbonate (CO~3~^2-^) is a polyatomic ion**  Polyatomic Ions - Glass Test Tube and Beakers **Part 4.5: Polyatomic Ions EXTENSION** **[Ionic Formula]** **[Polyatomic ion name]** --------------------------------- --------------------------------------- OH^-^ Hydroxide NO~2~^-^ Nitrite NO~3~^-^ Nitrate ClO~2~^-^ Chlorite ClO~3~^-^ Chlorate HCO~3~^-^ Bicarbonate C~2~H~3~O~2~^-^ Acetate CO~3~^2-^ Carbonate SO~3~^2-^ Sulphite SO~4~^2-^ Sulphate PO~4~^3-^ Phosphate NH~4~^+^ Ammonium **[Chemical Formula that include Polyatomic Ions]** 1. Determine the names of the following ionic compounds using names in the table below: a. Ba(NO~3~)~2~ *Barium Nitrate* b. NaNO~2~ c. K~2~CO~3~ d. MgSO~4~ e. Mg(OH)~2~ f. NaHCO~3~ g. NH~4~Cl 2. Determine the formula for following: a. Potassium Nitrate b. Barium Carbonate c. Sodium Acetate d. Aluminium Phosphate **Part 4.5: Polyatomic Ions EXTENSION** **[Challenge: Chemical Formula that include Polyatomic Ions]** **Determine the chemical formula for the following ionic compounds. A few have been done for you.** (Remember the cross-over rule. And remember to put polyatomic ions in brackets when needed). A picture containing pie chart Description automatically generated  **\ ** **Part 5: Metallic Bonding** **Metallic bonding** is a type of chemical bonding that takes place between two **[metals]** 1. Metal atoms usually have \ 1. Draw a diagram to illustrate a metallic bond and a "sea" of free electrons 2. Explain how metallic bonds enable the following properties of metals: a. Conducts Electricity b. Malleable & Ductile 3. Steel is made of Iron and Carbon. Explain why steel is not formed with a metallic bond, and state what type of substance it is instead. **Part 6:** **Groups and Trends in the Periodic Table** **[Groups and Trends on the Periodic Table\ ]** **Analytical Chemistry** **[Analytical Chemistry]** ***\*Use the flowchart on the back\**** Table Description automatically generated Explain what indications would tell you that your unknown substance is Sodium Chloride? Explain what indicators would tell you that your unknown substance was ZnCO~3~?