The Periodic Table Chemistry Textbook

The Periodic Table Unit B - Section 2.2  Mendeleev and the First 63 Dmitri Mendeleev took the first 63 known elements and arranged them based on patterns in their properties and compositions. He then noticed spaces in the table and anticipated that elements would be found that...

The Periodic Table Unit B - Section 2.2  Mendeleev and the First 63 Dmitri Mendeleev took the first 63 known elements and arranged them based on patterns in their properties and compositions. He then noticed spaces in the table and anticipated that elements would be found that fit perfectly into the table.  Understanding the Periodic Table Horizontal rows are called periods. Vertical rows are called families or groups. Families share similar properties.  Individual Elements The individual symbols and numbers around an element each have important information. 9 1- F Fluorine ATOMIC ELEMENT SYMBOL NAME 19.998  Atomic Number 9 1- The atomic F Fluorine number tells ATOMIC you how many NUMBER protons (+) are 19.998 in one atom of that element. The atomic number also tells you the number of electrons (-) in each atom. This is because all atoms are neutral so they have an equal amount of positively and negatively charged particles.  Atomic Mass 9 1- Total number of F Fluorine protons and neutrons. 19.998 Atomic mass - # of protons = # of ATOMIC neutrons MASS  Ionic Charge The ionic charge shows how 9 1- many electrons the atoms will F Fluorine lose or gain in a chemical reaction. IONIC CHARGE Fluorine has gained an electron (-) so it now has an 19.998 extra negative charge.  Ionic Charge Here, Sodium has 11 1+ Na Sodium lost one electron so it now has a positive IONIC charge of 1. CHARGE 22.990  Periodic Patterns The periodic table contains patterns related to the properties of elements. See page 126 - 127 in your textbook.  Periodic Patterns Green elements Orange elements are Purple elements are metals. non-metals. are metalloids. -Shiny -Dull -Mix of metal and -Malleable -Brittle non-metal -Do not conduct -Conduct properties. electricity (except Electricity Carbon). Also called insulators. Can be solid or gas.  Groups/ Families Groups & Families are Vanadium numbered 1 - 18 and are Family usually called by the 1st element in their column. Example: Group 5 is the Vanadium family.  Important Groups To Know GROUP 1 GROUP 2 Alkali Metals Alkali Earth Metals Highly Reactive. Not as reactive as React with exposure Alkali Metals. to oxygen or water. GROUP 17 GROUP 18 Halogens Noble Gases Most reactive Most stable and non-metal elements. unreactive elements. Mrs. Hill opens a sealed jar that contains a strip of metal. As she does this it immediately ignites. This metals is likely in which family?  Drag each pin to the corresponding spot on the periodic table element. Atomic Number 12 2+ Mg Indicates lost or gained Magnesium electrons in reactions Not shown Number of neutrons on image. Number of electrons 24.305 Number of protons Matter and Chemical Change Unit B - Section 1.1 + 1.2  Quick Refresher! Which of the following is not a state of matter?  Pure Substances ELEMENTS Pure substances only contain one type of particle. 2 types: Elements on the periodic table → Gold, Carbon, Oxygen COMPOUNDS Compounds → Every molecule looks the exact same. (H2O, CO2, etc.)  Mixtures MECHANICAL MIXTURE Substances that are not pure are mixtures. Mechanical: Have visibly different components. → Also known as heterogenous mixtures SOLUTION Solutions: Look like one substances but are made of different particles. → Also known as homogeneous mixtures  Other Types of Mixtures Suspensions: cloudy mixtures where tiny particles of one substance are suspended within another. They separate over time. → Tomato juice Colloids: similar to suspensions but they do not separate easily. → Milk Matter can be classified as one of 3 states: -solid -liquid -gas To change the state of a substance we must add or remove energy.  Properties All types of matter have their own properties. There are 2 types of properties: -Physical -Chemical  Physical Properties Physical properties describe the appearance and structure of the substance. Melting Point Boiling Point Hardness Malleability Ductility Crystal Shape Solubility Density Conductivity Colour Lustre  Chemical Properties Chemical properties describe how substances interact with other substances.  Check in! What is the change from solid to gas called?  One More... A student explains that opened a vial of clear liquid and upon contact with air it immediately burst into flames. What he is describing is an example of what type of property? Check and Reflect Page 104- #1-10 Do not do #11 Observing Change in Matter Unit B- Section 1.3  Types of Changes PHYSICAL CHANGE Physical change: a change in the state of matter. This does not alter the particles of the substance. CHEMICAL CHANGE Chemical change: 2 or more materials react to create a new substance with different properties from the original substance.  Chemical Changes These are some primary examples of chemical change: CHANGE IN COLOUR FORMATION OF A NEW SOLID OR GAS RELEASE OR ABSORPTION CHANGE IN ODOR OF HEAT Freeze Drying Freeze drying removes up to 90% of the moisture in food. This means it can be kept for much longer. All you need to do is add water. One substance, Many Outcomes Scientists can take a common material and turn it into many things. Corn can be made into pop bottles, nail-polish remover and sometimes, fuel for cars. When corn is fermented it undergoes a chemical change and now has more uses. Corn products are mostly biodegradable. Name one kind of chemical change that you have already used today. Name 2 indicators of chemical change. Section Review Page 110-111 #1-17  Evolving Theories of Matter Unit B- Section 2.1  Science involves constantly re-evaluating our beliefs based on observation. Theories change over time. Stone Age Chemists The first chemists lived about 10,000 years ago. They only had stone tools because metals had not been discovered. Once they learned how to make fire they could manipulate substances or create new ones! They cooked, fire-hardened, and toughened materials.  EARLY INTEREST Around 7000 years ago people IN METALS discovered metals and these AND immediately became valuable. LIQUID MATTER Gold was shiny and did not tarnish Copper was used to pots, coins, and tools and became one of the elements in bronze.  The Iron Age Around 1200 B.C. people called the hittites discovered how to get iron from rocks. Iron + Carbon → Steel Cultures also started REALLY BIG mummifying bodies using DEAL! resin from plants.  The Atom Emerges About 2500 years ago, people recognized that rocks could be broken into very small pieces. How small could particles get? Democritus started an idea that the smallest particle was called “atomos” which was Greek for “indivisible”. Each material was made of its own “atomos”.  DEMOCRITUS AND THE ATOM DEMOCRITUS BELIEVED: -Atoms are hard particles -Made from one material in different forms & sizes -Continuously move and join together to make different substances  FROM ALCHEMY TO CHEMISTRY FOR 2000 YEARS AFTER DEMOCRITUS’ THEORY, PEOPLE PRACTICED ALCHEMY. ALCHEMY WAS PART MAGIC- PART SCIENCE ○ NOW CONSIDERED A PSEUDOSCIENCE. ○ THEY BELIEVED IT WAS POSSIBLE TO TURN ANYTHING INTO GOLD. ○ THEY PERFORMED SOME OF THE FIRST CHEMISTRY EXPERIMENTS.  New Interest in Atoms Alchemy never ended up working. So from the 1500s on, people explored further about the nature of matter. Robert Boyle Experimented with gases (Boyle’s Law) Agreed that all matter was made of tiny particles.  CHEMISTRY AS A SCIENCE In the 1770s, Antoine Laurent Lavoisier studied chemical interactions and came up with universal names for substances! Now scientists in different countries could share ideas in a universal language! Using his system, he named Hydrogen, Oxygen, and Carbon.  John Dalton John Dalton decided all matter was made of elements. Elements were pure substances and couldn’t be divided into different substances. Atoms of the same element = identical Matter could not be created or destroyed.  J. J. Thompson First person to discover a subatomic particle (particles smaller than atoms). Experimented to find negatively charged particles called electrons.  Thompson’s Theory Atoms contain electrons which are negatively charged particles. They sat inside a positively charged sphere. Also called the “raisin bun” model. Ernest Rutherford In 1912 Rutherford discovered the nucleus. This was the centre of the atom. He also discussed the proton (a positively charged particle like an electron). He believed electrons travelled around the nucleus. So Thompson had been ½ right. Neils Bohr In 1913 Neils Bohr discovered electron shells. -Electrons travel around the nucleus in orbits with fixed distances. -Electrons could jump from shell to shell by losing or gaining energy. Bohr’s Theory 1. Atoms are composed of 3 subatomic particles: -Electron (-) -Neutron (neutral) -Proton (+) 2. Protons and neutrons were found in the nucleus of the atom. 3. Electrons rotate around the nucleus.  Current Atomic Theory 1.Atoms are composed of Electrons (-) Protons (+) Neutrons (neutral) Just like 2. Protons and neutrons Bohr said! are found in the nucleus. Electrons circle the nucleus.  Current Atomic Theory 4. The number of 3. In stable atoms the protons an atom has # of protons and tells you what electrons is equal. element it is and identifies the atomic number.  Current Atomic Theory 5. The combined number of protons and neutrons tells you the atomic mass. 6. Valence electrons are the outermost ELECTRON CLOUD MODEL electrons of an atom. CHECK THIS OUT! Atomic Model Brainpop!  Connect the scientist with their atomic model or theory by drawing lines. Dalton Bohr Thompson Rutherford All atoms of the same Discovered element look the exact the proton. same.  Which of the following is not a subatomic particle? A: Proton, B: Electron, C: Neutron, D: Phasar CHECK AND REFLECT PAGE 121- # 1-11