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Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table & Compounds Topic Using the Periodic Table Metals, NonMetals & Metalloids “I can…” Explain and identify the periods of the Periodic Table. Explain and identify the groups or families of the Periodic Table. Identify Elements by their symbol and their name. State the Atomic Number, Mass Number and Atomic Mass for any element, given the Periodic Table. State how many protons, neutrons and electrons are in an element, given the Periodic Table. Explain what an isotope is. State the Atomic Mass, Mass Number, Number of Neutrons, Protons and Electrons for an isotope of an element. Explain how an ion is formed. State the ion charge of an element, given the Periodic Table. Identify Metals on the Periodic Table. State the physical properties of most metals. State the chemical properties of most metals. Identify Non-Metals on the Periodic Table. State the physical properties of most non-metals. State the chemical properties of most non-metals. Identify Metalloids on the Periodic Table. Element Families Classification of Matter Types of Compounds Compound Symbols State the physical properties of most metalloids. State the chemical properties of most metalloids. Identify the Alkali Metals; explain their similarities and differences. Identify the Alkaline-Earth Metals; explain their similarities and differences. Identify the Halogens; explain their similarities and differences. Identify the Noble Gases; explain their similarities and differences. Distinguish between Pure Substances and Mixtures; give examples of both. Distinguish between Compounds and Elements; give examples of both. Distinguish between Homogeneous Mixtures and Heterogeneous Mixtures; give examples of both. Explain how a solid solution can exist and give an example of a solid solution. Explain the properties of Ionic Compounds. Explain how the atoms are bonded in Ionic Compounds. State which types of atoms create Ionic Compounds. Explain the properties of Molecular Compounds. Explain how the atoms are bonded in Molecular Compounds. State which types of atoms create Molecular Compounds. Explain what atoms create Diatomic Molecules. State any elements are in a compound, given the symbolic formula. State the quantity of elements within a compound, given the symbolic formula. Sketch a rough diagram of each compound. Explain how no atoms are lost in a chemical change; that the mass and the atoms balance going into a reaction and coming out of a reaction. 4.1 - Using the Periodic Table _________________ knew that some elements were very similar, and it made sense to him to group them together. For example, he grouped together _____________, _____________, and other metals that reacted violently with _____________. In 1886, the element _____________was discovered. This element had the exact properties of a __________________________on Mendeleev’s table. __________________________rearranged the elements to the table we have now based on the __________________of the elements. Label the following onto the blank periodic table: - Periods, groups - Solid, liquid, gas - Metal, metalloid, non-metal - Alkali Metals, Alkaline Earth metals, Halogens, Nobel Gases, Transitional Metals Use the Sask. Science 9 (pg 177-187) to complete the notes below: Period - _________________ row of elements in the periodic table - They are numbered from _____ to _____ - The most ___________ metals start on the ___________, as you move __________ the metals become less reactive Group/Family - _________________ column of elements in the periodic table - They are numbered from _____ to _____ - Elements in the same group have ______________________ Element Symbol & Name (Pg 160 – 161) - Element symbols are used to describe elements because ___________________________ __ and it will make ________________________ - An element symbol consists of _____ or _____ letters - The ____________ letter is capitalized, and if there is a second letter it is ________________ - The rule about capitalization is very important. Ex. The symbol _________ stands for _____________, while _______ represents ________________ (a compound that contains both ___________ and _____________) - The symbol is sometimes an __________________ of the elements English name, other times it abbreviates the elements ______________ name. Ex/ the symbol for Silicone is _______ where as the symbol for Silver is ______ because its Latin name is _____________. - Some elements are named based on where they were discovered, like _______________ which was discovered at the University of California. - _________________ is a strong yet light metal element. It is named for the ___________, powerful gods of Greek mythology. Atomic Number - The atomic number is typically found _______________________ of each element square - It shows how many ___________ are in one atom of that element. - Atoms have a ____________ charge, therefore the number of __________________ equals the number of __________________ - As you move across the periodic table from left to right the atomic number _____________ by ___________ Ex/ Nickel’s atomic number is____________, therefore it has _____________ protons and ______________ electrons Atomic Mass - Typically found ___________ the elements name in each element square - Atomic mass is always expressed as a _____________, because each element, except for _____________, can form _____________, which are atoms with different numbers of ____________ in them and therefore different ______________. - Atomic mass is the average _____________of all an element’s different _____________ - Mass is measured in _____________ _____________ _____________ (amu) - Hydrogen has an atomic mass of _____________and iron has an atomic mass of _____________. This means that iron is _____________times heavier than hydrogen atoms. Mass Number The mass number of an element is the atomic number rounded to a whole number - Is the total number of ______________ and ________________ in an atom - __________ are too small, therefore they have very little effect on the total mass of the atom - To determine the number of neutrons an element has subtract the _______________ from the ________________ ___________________ - __________________ = ____________________ Isotopes - A form of an atom that has a different number of _____________than the common form of that atom - Ex. The most common form of hydrogen has _____________proton and _____________ electron but _____________neutrons. A small percentage of hydrogen atoms have _____________ proton, _____________electron, and _____________neutron. An even smaller percentage of hydrogen atoms have _____________proton, _____________electron and _____________ neutrons. - The most common form of carbon contains _____ protons and _______ neutrons, therefore has a mass number of _________. Carbon-14 is an isotope of carbon that has a mass number of 14. Because it isn’t the most common form of carbon, its mass number is indicated with “-14” at the end of the element name. Carbon-14 is used for _____________________ Ion Charge - Ions are formed when atoms or groups of atoms _____________or _____________electrons. - Ion charge is the _____________charge that an atom takes on when it loses or gains electrons. - Elements that gain electrons become _____________charged, whereas elements that lose electrons become _____________charged. - Elements with atoms that form similar _____________are grouped together in the periodic table. For example, elements in the first column on the left side of the periodic table all form _____________ions of ion charge _____________. Complete the table below: Element Element Atomic Atomic Mass Ion # of # of # of Name Symbol Number Mass Number Charge Protons electrons neutrons Hydrogen Bromine – 81 Iron Titanium-46 Lead Uranium-235 Vanadium Phosphorus Argon Magnesium Uranium Carbon Helium Assignment: Complete Chart above and complete questions from Saskatchewan Science 9 page 188#3, 4, 8. 4.2 – Metals, Non-metals, Metalloids Metals - Metals are found of the ______________ side of the periodic table Physical Properties o Most are ____________ and ______________ o Excellent conductors of ___________ and ___________ o They are also ______________ and _________________ o Most metals are ____________ at room temperature. ______________ is a metal that is ______________ at room temperature. Chemical Properties o Some metals react explosively with ____________ (Ex. ______________) o Others will not react even if mixed with ________________ (Ex. ______________) Non – Metals - Only __________ of the known elements are classified by scientists as non-metals. - These elements are not grouped because of their similarities but because _______________________________ - Non-Metals are found of the ______________ side of the periodic table Physical Properties - __________of the non-metals are gases at room temperature, _________ are solid, and ________ is liquid. - Solid non-metals do not conduct _____________or ____________. - Solid non-metals are ____________________ and not ____________________ elements - Solid non-metals have little or no ________________ Chemical Properties - Some non-metals are very reactive. - _____________ is a Yellow solid. It is a very reactive _____________ gas and will ________ in air. It will melt into a liquid with __________ heat. - Pure _________________ is very _____________ and ______________. Metalloids - Have both _______________ and ________________ properties - They are often used in _________________, such as __________________ Physical Properties - Metalloids ______________ electricity but _______________, they are called _______________ - _________________ is the most common metalloid. It is _____________ and ___________, but unlike a metal, it is ____________. About 40% of the mass of any _____________ comes from silicon. It is also a major component in _______________ Assignment: complete questions from Saskatchewan Science 9 page 165 #1, 3, 6, 7. 4.3 – Element Families Alkali Metals - Group ______ elements. Similarities - _____________in colour. - Like other metals, they are _____________ and _____________; they conduct _____________and _____________. - Unlike other metals, they have _____________melting points and melt below _____________ - These are the ___________________ metals. - These metals react when exposed to ______________ or _____________ Differences - From top to bottom, _____________increases, and _____________decreases. Alkaline-Earth Metals - Group ______ elements - _____________in colour. - These elements also react when exposed to __________ or ____________, however their reactivity is not as _______________ as alkali metals - They are _____________ and have a _____________ than sodium and potassium - Alkaline-Earth Metals have _____________ melting points that alkali metals Halogens - Group _____ elements Similarities - Each has a _____________ but _____________ colour. - They all have a low _____________ point - They are the most ____________ non-metals Differences - Moving from top to bottom, the colours of the vapours grow in _____________ - Also, melting points _____________ Noble Gases - Group ______ elements Similarities - All exist naturally as _____________ gases, but will glow with bright colours if _______________________________________ - They are the most ___________________ elements Differences - From top to bottom, the _____________ increases Assignment: complete questions from Saskatchewan Science 9 page 184 #1-3. 4.4 - Classification of matter All __________ _______________ ____________________ - Contain only one type of particle - can exist in three __________ ___ __________: solid, liquid and gas _______________ - Examples: water, salt, _______________ - contain two or more pure substances _______________ _________________ _________________ (Solutions) - Examples: iron, gold, oxygen - appear to be one substance sugar - particles of different substances are intermingled - examples: vinegar, clear air _________________ _________________ (Mechanical Mixtures) - two ore more parts can be seen - different kinds of particles stay together - examples: soil, blood, concrete _____________ Identify each mixture as homogeneous or heterogeneous. Dirt____________ Sterling silver bracelet ________________ Sample of pond water _______________ Recycled paper ________________ Answer each question with a full sentence. To the unaided eye, a mixture appears to be a white liquid with no visible substances floating around. Can this mixture be classified as homogeneous? Explain why or why not. Air can be classified as heterogeneous or homogeneous. Explain why this statement is true. Read the descriptions below. In the space provided, indicate whether each mixture is a mechanical mixture (MM) or a solution (S) The different substances in this mixture can be distinguished from each other with the unaided eye or a magnifying glass _______ The substances in this mixture cannot be separated by filtering________ When this mixture is left to stand undisturbed, the substances do not separate by floating to the top or settling to the bottom. ________ This mixture appears cloudy or opaque. You cannot see through it clearly. ______ Combining Metals (Pg 159) Some metals, such as __________ and ___________, are too ___________ to be used alone for some purposes. Therefore, to make a substance stronger, some metals are often melted and mixed with other melted metal elements. The mixture is cooled to become a solid ____________. A solution of two or more metals is called an ____________. Common alloys include a combination of ____________ and _____________ or _____________, this is often called ________________ because it has a lighter colour than pure gold. White gold is often used in engagement rings and wedding bands to give them ______________ and _______________. Alloys are used in _____________, __________________, ______________ and many other household items. Assignment: complete questions from Saskatchewan Science 9 page 127 #2-4, 7 and page 146 #3, 15. 4.5 –Types of Compounds Ionic Compounds Properties - Ionic compounds have ______________ melting points (they are solid at room temperature) - When dissolved in water, they are good ______________ - They all form ______________ How they are formed - - Ionic compounds are pure substances formed as a result of the attraction between ions of opposite charges ______________ atoms tend to lose electrons, therefore they become ______________ ions. Whereas, ______________atoms tend to gain electrons, therefore they become ______________ ions. Ex) When ______________ combines with ______________, an electron from the highest energy level of a sodium atom moves to the outer level of the chlorine atoms. This causes the atoms to become ______________. Molecular Compounds - Composed of 2 ______________ - May be ______________, ______________ or ______________ at room temperature - Tend to be ______________ or poor conductors of electricity - They have relatively ______________ melting and boiling points due to the weak forces between molecules - In a molecular compound, atoms join together by ______________ electrons in the highest energy level Diatomic Molecules - Molecules composed only of ________ ___________ are _______________ ___________________. Common diatomic molecules are ______________, _____________, ________________, _____________________, ____________________, ___________________, _________________, and _______________________. Assignment: complete questions from Saskatchewan Science 9 page 173 #1-4, 9. 4.6 – Compound Symbols Physical State of Compounds - Commonly a chemicals state ___ _____________ ________________ will be indicated behind the element compound as a subscript, ____ – solid, _____ – liquid, _____ – gas, _____ – aqueous (dissolved in water) Symbols - The symbol of each ____________ that is contained in a compound will be written in the _______________ _____________________ of that compound Ex/ NaCl ***Remember – there are 1 or 2 letters in each compound symbol and the first letter is capitalized, the second is lowercase Therefore the two symbols in NaCl are Na and Cl, which means that ________________ and ____________ are contained in NaCl - There are sometimes ________________ behind a chemical symbol, these numbers show how many ___________ of each chemical are in the compound. Ex/ H2O 2 Hydrogen and 1 Oxygen molecule Complete the table below Compound Element in compound CaO Molecular or Ionic Number of Atoms Drawing of Compound in Each Element CaCl2 Al2O3 Na2O AlCl3 NaOH Chemical Formula - Matter cannot be ____________________ ____ ______________________. - In _____________ ___________________, both sides must contain the same number of atoms of each ___________________. - _____________ _________________ in front of a compound indicate how many ____________ of the compound are used in the _____________ ___________. Ex/ 2CH3OH + 3O2 -2CO2 + 4 H2O In CH3OH, there is ____ carbon, _____ Hydrogen, and ____ Oxygen and in O2 there are ____ oxygen. The formula uses _____ of CH3OH molecules and 3 _____, therefore on the left side of the formula… 2 – Carbon 8 – Hydrogen 8 – Oxygen On the left side of the equation, there are 2 molecules of CO2 and 4 molecules of H2O. Therefore there are: 2 – Carbon 8 – Hydrogen 8 – Oxygen - In addition to matter being conserved, the ________ is also conserved. Ex/ Mg + S MgS 24.3g 32.1g 56.4 Assignment: complete questions from Saskatchewan Science 9 page 173 #7, 11.