2012 chapter 4 study guide
... The organization of the periodic table is based on the properties of the elements and reflects the structure of atoms. As a basis for understanding this concept: 7 a. Students know how to identify regions corresponding to metals, nonmetals, and inert gases. Be able to 7. tell who Mendeleev was and h ...
... The organization of the periodic table is based on the properties of the elements and reflects the structure of atoms. As a basis for understanding this concept: 7 a. Students know how to identify regions corresponding to metals, nonmetals, and inert gases. Be able to 7. tell who Mendeleev was and h ...
SCH3U Periodic Table Worksheet 1. Where are the most active
... 1. Where are the most active metals located? Group 1. Also, the bottom periods of the periodic table. 2. Where are the most active non-metals located? Top right of the periodic table. Fluorine being the highest. Group 17 very reactive. 3. As you go from left to right across a period, the atomic radi ...
... 1. Where are the most active metals located? Group 1. Also, the bottom periods of the periodic table. 2. Where are the most active non-metals located? Top right of the periodic table. Fluorine being the highest. Group 17 very reactive. 3. As you go from left to right across a period, the atomic radi ...
Periodic Table Powerpoint
... Noble Gases are colorless gases that are extremely unreactive. One important property of the noble gases is their inactivity. They are inactive because their outermost energy level is full. Because they do not readily combine with other elements to form compounds, the noble gases are called inert. T ...
... Noble Gases are colorless gases that are extremely unreactive. One important property of the noble gases is their inactivity. They are inactive because their outermost energy level is full. Because they do not readily combine with other elements to form compounds, the noble gases are called inert. T ...
Structure of Atoms/Periodic Table Review 1. Shade in location of the
... 20. Why are atoms neutral? They have the _________ __________ of protons and neutrons. 22. What are the limitations of the Bohr model? ____________ do not orbit the nucleus like planets orbit the sun. The ___________ does not represent the actual size of an atom. 23. What determines an element’s ide ...
... 20. Why are atoms neutral? They have the _________ __________ of protons and neutrons. 22. What are the limitations of the Bohr model? ____________ do not orbit the nucleus like planets orbit the sun. The ___________ does not represent the actual size of an atom. 23. What determines an element’s ide ...
Chapter 5 student
... of elements in those groups. • Predict the reactivity of some elements based on their locations within a group. • Identify some properties of common A group elements. ...
... of elements in those groups. • Predict the reactivity of some elements based on their locations within a group. • Identify some properties of common A group elements. ...
Jeopardy
... a. good conductors of thermal energy. b. more reactive than alkali metals. c. not good conductors of electric current. d. used to make aluminum. ...
... a. good conductors of thermal energy. b. more reactive than alkali metals. c. not good conductors of electric current. d. used to make aluminum. ...
the periodic table
... CHEMISTRY TEST REVIEW Use this as a study tool to review for your CCA, October 18 th. ...
... CHEMISTRY TEST REVIEW Use this as a study tool to review for your CCA, October 18 th. ...
The Periodic Table Worksheet
... 4. a) What is the link between the group to which an element belongs in the periodic table and the number of electrons in an atom of the element’s outer shell? ...
... 4. a) What is the link between the group to which an element belongs in the periodic table and the number of electrons in an atom of the element’s outer shell? ...
Periodic Table Worksheet
... 8. As you go down a group, the first ionization energy generally (DECREASES / increases). Why? OUTERMOST ELECTRON IS FARTHER AWAY FROM NUCLEUS; SHIELDING EFFECT OF INNER ELECTRONS. 9. Where is the highest electronegativity found? UPPER RIGHT (F) 10. Where is the lowest electronegativity found? LOWER ...
... 8. As you go down a group, the first ionization energy generally (DECREASES / increases). Why? OUTERMOST ELECTRON IS FARTHER AWAY FROM NUCLEUS; SHIELDING EFFECT OF INNER ELECTRONS. 9. Where is the highest electronegativity found? UPPER RIGHT (F) 10. Where is the lowest electronegativity found? LOWER ...
Periodic Table Funsheet (KEY) 1. Where are the most active metals
... 8. As you go down a group, the first ionization energy generally (DECREASES / increases). Why? OUTERMOST ELECTRON IS FARTHER AWAY FROM NUCLEUS; SHIELDING EFFECT OF INNER ELECTRONS. 9. Where is the highest electronegativity found? UPPER RIGHT (F) 10. Where is the lowest electronegativity found? LOWER ...
... 8. As you go down a group, the first ionization energy generally (DECREASES / increases). Why? OUTERMOST ELECTRON IS FARTHER AWAY FROM NUCLEUS; SHIELDING EFFECT OF INNER ELECTRONS. 9. Where is the highest electronegativity found? UPPER RIGHT (F) 10. Where is the lowest electronegativity found? LOWER ...
Periodic Table Funsheet (KEY) 1. What family has the most active
... 14. Group 17 elements are called HALOGENS. 15. Group 18 elements are called NOBLE GASES. 16. As you go from left to right across the periodic table, the elements go from (METALS / nonmetals) to (metals / NONMETALS). 17. The most active element in Group 17 is FLUORINE. 18. What sublevels are filling ...
... 14. Group 17 elements are called HALOGENS. 15. Group 18 elements are called NOBLE GASES. 16. As you go from left to right across the periodic table, the elements go from (METALS / nonmetals) to (metals / NONMETALS). 17. The most active element in Group 17 is FLUORINE. 18. What sublevels are filling ...
Unit 1 Topics to Review
... Energy levels hold a certain number of electrons. There are 7 energy levels, they are shown as periods on the Periodic Table of Elements. The history of the Periodic Table. Know that there are Groups 1-18 on the Periodic Table, and be able to find them. There is a staircase that separates metals and ...
... Energy levels hold a certain number of electrons. There are 7 energy levels, they are shown as periods on the Periodic Table of Elements. The history of the Periodic Table. Know that there are Groups 1-18 on the Periodic Table, and be able to find them. There is a staircase that separates metals and ...
Unit 2 Periodic Table
... Atoms of this family have 6 valence electrons. Known as chalcogen family. Most elements in this family share electrons when forming compounds. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements. ...
... Atoms of this family have 6 valence electrons. Known as chalcogen family. Most elements in this family share electrons when forming compounds. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements. ...
Atom/Elements Study Guide
... The atom is the smallest particle that cannot be broken down by ordinary means; it is the building block of all matter. A neutral atom is one that carries no charge because the protons (+) and electrons (-) are equal, therefore balancing each other out. Elements are the simple building blocks of all ...
... The atom is the smallest particle that cannot be broken down by ordinary means; it is the building block of all matter. A neutral atom is one that carries no charge because the protons (+) and electrons (-) are equal, therefore balancing each other out. Elements are the simple building blocks of all ...
Textbook Questions - Teach-n-Learn-Chem
... 2. List two reasons why Mendeleev is given more credit than Meyer for creating the periodic table. ...
... 2. List two reasons why Mendeleev is given more credit than Meyer for creating the periodic table. ...
CHMB homework Name © Van Der Sluys, 2004 Periodic Table 1
... 5. A negative ion is (larger/smaller) that its parent atom and a positive ion is (larger/smaller) than its parent atom. 6. From left to right across a period, the first ionization energy (decreases/increases). 7. As you go down a group, the first ionization energy (decreases/increases). 8. What elem ...
... 5. A negative ion is (larger/smaller) that its parent atom and a positive ion is (larger/smaller) than its parent atom. 6. From left to right across a period, the first ionization energy (decreases/increases). 7. As you go down a group, the first ionization energy (decreases/increases). 8. What elem ...
The Periodic Table - Lincoln Park High School
... • Elements in groups 3-12 • Less reactive harder metals • Includes metals used in jewelry and construction. ...
... • Elements in groups 3-12 • Less reactive harder metals • Includes metals used in jewelry and construction. ...
2.2 The Periodic table and Chemical Properties
... • This is the average mass of an atom of an element. • It is always written as a decimal number and is measured in atomic mass unit (amu) ...
... • This is the average mass of an atom of an element. • It is always written as a decimal number and is measured in atomic mass unit (amu) ...
Chapter 6 Periodic law- states that when the elements are arranged
... Group- A vertical column of elements in the periodic table; also called a family Period- A horizontal row of elements in the modern periodic table Representative element- groups of elements in the modern periodic table that are designated with an A (1A-8A) and possess a wide range of chemical and ph ...
... Group- A vertical column of elements in the periodic table; also called a family Period- A horizontal row of elements in the modern periodic table Representative element- groups of elements in the modern periodic table that are designated with an A (1A-8A) and possess a wide range of chemical and ph ...
Name Periodic Table Assignment Directions: Using your text (pgs
... 3. Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element X be found? ...
... 3. Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element X be found? ...
Chapter 4 Notes - Riverton High School
... Atoms of this family have 6 valence electrons. Most elements in this family share electrons when forming compounds. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements. ...
... Atoms of this family have 6 valence electrons. Most elements in this family share electrons when forming compounds. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements. ...
Name: Date: _____ Pd: _____ Chemistry, PERIODIC TABLE Spring
... energy generally increases. (2) The atomic radius decreases, and the first ionization energy generally decreases. (3) The atomic radius increases, and the first ionization energy generally decreases. (4) The atomic radius increases, and the first ionization energy generally increases. ...
... energy generally increases. (2) The atomic radius decreases, and the first ionization energy generally decreases. (3) The atomic radius increases, and the first ionization energy generally decreases. (4) The atomic radius increases, and the first ionization energy generally increases. ...
Name: Homeroom
... on the substance. Adding or removing heat cause changes in state. The increase or decrease of decrease on a substance can also cause changes in states of matter. Melting Point: temperature at which a substance changes from a solid to a liquid. Boiling Point: temperature at which a substance changes ...
... on the substance. Adding or removing heat cause changes in state. The increase or decrease of decrease on a substance can also cause changes in states of matter. Melting Point: temperature at which a substance changes from a solid to a liquid. Boiling Point: temperature at which a substance changes ...
Period 2 element
The period 2 elements are the chemical elements in the second row (or period) of the periodic table. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behavior of the elements as their atomic number increases; a new row is started when chemical behavior begins to repeat, creating columns of elements with similar properties.The second period contains the elements lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon. This situation can be explained by modern theories of atomic structure. In a quantum mechanical description of atomic structure, this period corresponds to the filling of the 2s and 2p orbitals. Period 2 elements obey the octet rule in that they need eight electrons to complete their valence shell. The maximum number of electrons that these elements can accommodate is ten, two in the 1s orbital, two in the 2s orbital and six in the 2p orbital. All of the elements in the period can form diatomic molecules except beryllium and neon.