Unit 13
... C Mendeleev eventually produced the first periodic table of the elements. C He arranged his table so that elements in the same column have similar properties. C He switched the order of three pairs of elements so as to keep elements in columns with similar properties. C He boldly pronounced that per ...
... C Mendeleev eventually produced the first periodic table of the elements. C He arranged his table so that elements in the same column have similar properties. C He switched the order of three pairs of elements so as to keep elements in columns with similar properties. C He boldly pronounced that per ...
Chapter 4
... When ___________ react, they often __________ the one electron needed to have eight valence electrons, a filled outer energy level. ...
... When ___________ react, they often __________ the one electron needed to have eight valence electrons, a filled outer energy level. ...
Chapter 5 - The Periodic Law
... Periods and the Blocks of the Periodic Table A. Periods 1. Horizontal rows on the periodic table 2. Period number corresponds to the highest principal quantum number of the elements in the period B. Sublevel Blocks 1. Periodic table can be broken into blocks corresponding to s, p, d, f sublevels II. ...
... Periods and the Blocks of the Periodic Table A. Periods 1. Horizontal rows on the periodic table 2. Period number corresponds to the highest principal quantum number of the elements in the period B. Sublevel Blocks 1. Periodic table can be broken into blocks corresponding to s, p, d, f sublevels II. ...
Chapter_3_Fast_Facts
... Atomic radius: atomic radii decrease along a period as the nuclear charge increases and electrons are added to the same outer shell. The attraction between the outer electrons and nucleus increases. ...
... Atomic radius: atomic radii decrease along a period as the nuclear charge increases and electrons are added to the same outer shell. The attraction between the outer electrons and nucleus increases. ...
The Periodic Law Notes (Chapter 5) – Part 2
... 3. Group trend – ionization energy increases as you move up a group (or decreases as you move down a group). In general, as you do down a group the ionization energy decreases because the size of the atom is increasing and the outermost electrons are further from the nucleus. 1. Which atom has the h ...
... 3. Group trend – ionization energy increases as you move up a group (or decreases as you move down a group). In general, as you do down a group the ionization energy decreases because the size of the atom is increasing and the outermost electrons are further from the nucleus. 1. Which atom has the h ...
8th Science LF Sept 7-11
... Color the periodic table to distinguish location of metals, non-metals, and metalloids. Think Pair Share – Identify Periodic Table Trends Discover that Element Game from Discovery Education (print pgs. 2 and 10) Quick Write – See Critical Writing Prompt ...
... Color the periodic table to distinguish location of metals, non-metals, and metalloids. Think Pair Share – Identify Periodic Table Trends Discover that Element Game from Discovery Education (print pgs. 2 and 10) Quick Write – See Critical Writing Prompt ...
TEST-Periodic Table
... a. Rb is the most reactive element shown. Group 1A alkaline earth metals are the most reactive metals, and the reactivity of elements in Group 1A increases from top to bottom. b. Li is the most reactive element shown. Group 1A alkaline earth metals are the most reactive metals, and the reactivity of ...
... a. Rb is the most reactive element shown. Group 1A alkaline earth metals are the most reactive metals, and the reactivity of elements in Group 1A increases from top to bottom. b. Li is the most reactive element shown. Group 1A alkaline earth metals are the most reactive metals, and the reactivity of ...
File
... compounds similar to those of halogens such as CCl4 and CH4 Now due to these reasons hydrogens place is not decided .It is placed separately above alkali metals as a special elementjust because of same electronic configuration. Q10)Discuss the trends in properties in periods and groups. ( this qts w ...
... compounds similar to those of halogens such as CCl4 and CH4 Now due to these reasons hydrogens place is not decided .It is placed separately above alkali metals as a special elementjust because of same electronic configuration. Q10)Discuss the trends in properties in periods and groups. ( this qts w ...
The Periodic Law Notes (Chapter 5) – Part 2
... atoms get smaller. Another way to think of it: the number of valence electrons increases (the amount of energy needed to remove one electron is less then what is needed to remove 7 or 8 electrons). 3. Group trend – ionization energy increases as you move up a group (or decreases as you move down a g ...
... atoms get smaller. Another way to think of it: the number of valence electrons increases (the amount of energy needed to remove one electron is less then what is needed to remove 7 or 8 electrons). 3. Group trend – ionization energy increases as you move up a group (or decreases as you move down a g ...
Document
... a neighboring atom - tends to vary in different substances - For metals - atomic radius is defined as half distance between adjacent nuclei in a crystal of the element ...
... a neighboring atom - tends to vary in different substances - For metals - atomic radius is defined as half distance between adjacent nuclei in a crystal of the element ...
Periodic Table of Elements
... • Family 17 is known as the Halogen family. • They have 7 valence electrons and are the most reactive non-metals. • They only need to gain 1 electron and are not found as free atoms in nature. • They often combine with the transition metals. • Examples: Cl, I, and Br ...
... • Family 17 is known as the Halogen family. • They have 7 valence electrons and are the most reactive non-metals. • They only need to gain 1 electron and are not found as free atoms in nature. • They often combine with the transition metals. • Examples: Cl, I, and Br ...
Periodic Trends
... table, you can predict almost anything about any element on the periodic table. We will study: • Atomic Radii • Ionic Radii • Valence Electrons • Reactivity • Electronegativity • Electron Configuration ...
... table, you can predict almost anything about any element on the periodic table. We will study: • Atomic Radii • Ionic Radii • Valence Electrons • Reactivity • Electronegativity • Electron Configuration ...
An element
... Physical properties: Solid at room temperature but gets bent out of shape easily. Difficult to find a pure sample. Due to rust, aging samples are unable to conduct electricity as easily as young samples. Chemical properties: Attempts to bond with WO any chance it can get. Also tends to form strong b ...
... Physical properties: Solid at room temperature but gets bent out of shape easily. Difficult to find a pure sample. Due to rust, aging samples are unable to conduct electricity as easily as young samples. Chemical properties: Attempts to bond with WO any chance it can get. Also tends to form strong b ...
Periodic trends - poynette.k12.wi.us
... Prepare a graph of first, second, and third ionization energy vs. atomic number. 1. What is a kJ/mol? ...
... Prepare a graph of first, second, and third ionization energy vs. atomic number. 1. What is a kJ/mol? ...
Part B: Periodic Trends
... 14. What is the symbol of the element with the highest ionization energy? _______ 15. What element has the lowest electronegativity? _______ 16. Who was given credit for first developing the periodic table of the elements? ______________ 17. The energy that is required to remove an electron from it ...
... 14. What is the symbol of the element with the highest ionization energy? _______ 15. What element has the lowest electronegativity? _______ 16. Who was given credit for first developing the periodic table of the elements? ______________ 17. The energy that is required to remove an electron from it ...
The Periodic Table and Periodicity
... of each element and placed them in order of increasing atomic number, rather than atomic weight. This atomic number arrangement also followed Mendeleev’s trends in properties. Elements with similar properties were grouped together. The modern period table was born (1914). ...
... of each element and placed them in order of increasing atomic number, rather than atomic weight. This atomic number arrangement also followed Mendeleev’s trends in properties. Elements with similar properties were grouped together. The modern period table was born (1914). ...
Test Review
... Alkaline Earth Metals – Group 2, not as reactive as alkali metals. Form +2 ions, losing 2 electrons to look like a noble gas. Halogens – Group 7, most reactive metals on the periodic table. Form -1 ions, gaining 1 electron to look like a noble gas. Known as the salt formers, since they tend to bond ...
... Alkaline Earth Metals – Group 2, not as reactive as alkali metals. Form +2 ions, losing 2 electrons to look like a noble gas. Halogens – Group 7, most reactive metals on the periodic table. Form -1 ions, gaining 1 electron to look like a noble gas. Known as the salt formers, since they tend to bond ...
Chapter 13
... Periodic Trend – There is a decrease in the size of cations as you move across a period from left to right – when you get to group 4A the anions (which are much larger) start to decrease in size Group Trend – Ionic size (both cations and anions) increases as you go down each group. ...
... Periodic Trend – There is a decrease in the size of cations as you move across a period from left to right – when you get to group 4A the anions (which are much larger) start to decrease in size Group Trend – Ionic size (both cations and anions) increases as you go down each group. ...
the modern periodic law
... chlorine to form colourless compounds which crystallize in cubic shapes and have similar formulas: LiCl, NaCl, KCl, RbCl, CsCl, and FrCl. Halogens are elements of group 17. The word halogen means salt-former. All these elements have non-metallic properties. They react with hydrogen to form compounds ...
... chlorine to form colourless compounds which crystallize in cubic shapes and have similar formulas: LiCl, NaCl, KCl, RbCl, CsCl, and FrCl. Halogens are elements of group 17. The word halogen means salt-former. All these elements have non-metallic properties. They react with hydrogen to form compounds ...
Periodic Table Notes Ch. 6 ppt
... Because electrons are further from the nucleus, there is less attraction. Size (radius) goes DOWN on going across a period. ...
... Because electrons are further from the nucleus, there is less attraction. Size (radius) goes DOWN on going across a period. ...
word - My eCoach
... 7. The force of attraction that holds ions together in salts like KCl is ___________. a. electrostatic c. magnetic b. nuclear d. gravitational ...
... 7. The force of attraction that holds ions together in salts like KCl is ___________. a. electrostatic c. magnetic b. nuclear d. gravitational ...
Effective Nuclear Charge
... Within each period, the metals at the left form cations and the nonmetals at the right form anions. There is a decrease in the ionic radii of the cations from left to right and a decrease in the ionic radii of the anions from left to right. ...
... Within each period, the metals at the left form cations and the nonmetals at the right form anions. There is a decrease in the ionic radii of the cations from left to right and a decrease in the ionic radii of the anions from left to right. ...
III. Periodic Trends
... The ease with which an atom gains an e-. For most atoms, the energy released when an e- is added. (in kJ/mol) Periodic Trend 1. Electron affinity slightly decreases down a group. 2. Electron affinity generally tends to increase across a period. ...
... The ease with which an atom gains an e-. For most atoms, the energy released when an e- is added. (in kJ/mol) Periodic Trend 1. Electron affinity slightly decreases down a group. 2. Electron affinity generally tends to increase across a period. ...
Periodic Law
... groups of elements. Group I elements are called alkali metals. Group 2 elements are called alkaline earth metals. The nonmetals of Group 17 are called halogens. Group 18 elements are called Noble Gases Groups 3–12 are called transition metals The two periods usually located at the bottom of the peri ...
... groups of elements. Group I elements are called alkali metals. Group 2 elements are called alkaline earth metals. The nonmetals of Group 17 are called halogens. Group 18 elements are called Noble Gases Groups 3–12 are called transition metals The two periods usually located at the bottom of the peri ...
Bonding 1 - Deans Community High School
... Na to Al the atom size decreases leading to greater packing in metal lattice. Si is a covalent network, tightly packed atoms in covalent lattice. P and S are covalent molecular solids with quite densely packed molecules. Cl and Ar are covalent molecular gases at room temperature. ...
... Na to Al the atom size decreases leading to greater packing in metal lattice. Si is a covalent network, tightly packed atoms in covalent lattice. P and S are covalent molecular solids with quite densely packed molecules. Cl and Ar are covalent molecular gases at room temperature. ...
Period 3 element
A period 3 element is one of the chemical elements in the third row (or period) of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behaviour of the elements as their atomic number increases: a new row is begun when the periodic table skips a row and a chemical behaviour begins to repeat, meaning that elements with similar behavior fall into the same vertical columns. The third period contains eight elements: sodium, magnesium, aluminium, silicon, phosphorus, sulfur, chlorine, and argon. The first two, sodium and magnesium, are members of the s-block of the periodic table, while the others are members of the p-block. Note that there is a 3d orbital, but it is not filled until Period 4, such giving the period table its characteristic shape of ""two rows at a time"". All of the period 3 elements occur in nature and have at least one stable isotope.