Name - cloudfront.net
... When elements are arranged in the periodic table in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. The way properties change from left to right across a period and from top to bottom within a group are called periodic trends. Here is a su ...
... When elements are arranged in the periodic table in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. The way properties change from left to right across a period and from top to bottom within a group are called periodic trends. Here is a su ...
Slide 1
... 4. There are seven rows or periods on the periodic table. 5. Each period corresponds to a principle energy level. 6. There are more elements in higher number periods because there are more orbitals in higher energy levels. 7. Elements are also arranged in groups or columns of elements with similar p ...
... 4. There are seven rows or periods on the periodic table. 5. Each period corresponds to a principle energy level. 6. There are more elements in higher number periods because there are more orbitals in higher energy levels. 7. Elements are also arranged in groups or columns of elements with similar p ...
Unit 4 (2016 – 2017)
... There were places where heavier elements came before lighter elements because of properties: Te - I, ...
... There were places where heavier elements came before lighter elements because of properties: Te - I, ...
periodic law
... • Since there is a difference in electronegativity between the two elements (3.0 – 2.1 = 0.9), the bond in H–Cl is polar. • Since Cl is more electronegative, the bonding electrons are attracted toward the Cl atom and away from the H atom. This will give the Cl atom a slightly negative charge and the ...
... • Since there is a difference in electronegativity between the two elements (3.0 – 2.1 = 0.9), the bond in H–Cl is polar. • Since Cl is more electronegative, the bonding electrons are attracted toward the Cl atom and away from the H atom. This will give the Cl atom a slightly negative charge and the ...
Ch.6 Periodic Trends - MrsSavallisChemistry
... b. brittle c. malleable d. poor conductor of electric current e. shinny 5. In general, how are metalloids different from metals and nonmetals? 6. Elements in the same period have the same…? 7. Elements in the same group have similar…? 8. Based on their locations in the periodic table, would you expe ...
... b. brittle c. malleable d. poor conductor of electric current e. shinny 5. In general, how are metalloids different from metals and nonmetals? 6. Elements in the same period have the same…? 7. Elements in the same group have similar…? 8. Based on their locations in the periodic table, would you expe ...
17.3 The periodic table
... Elements on the same group have the same number of electrons in the outermost energy level. Since all members of a group on the peridic table have the same number of electrons in the outer energy level, group members will undergo chemical reactions in the same way. Elements on the same period ...
... Elements on the same group have the same number of electrons in the outermost energy level. Since all members of a group on the peridic table have the same number of electrons in the outer energy level, group members will undergo chemical reactions in the same way. Elements on the same period ...
Atoms and the Periodic Table Subatomic Particles
... – Increases in going across a period – Generally decreases in going down a group (some exceptions) ...
... – Increases in going across a period – Generally decreases in going down a group (some exceptions) ...
Chapter 11
... remove one mole of electrons from one mole of isolated gaseous atoms or ions. You may think of ionization energy as a measure of the difficulty of removing electron or the strength by which an electron is bound. The higher the ionization energy, the more difficult it is to remove an electron. Theref ...
... remove one mole of electrons from one mole of isolated gaseous atoms or ions. You may think of ionization energy as a measure of the difficulty of removing electron or the strength by which an electron is bound. The higher the ionization energy, the more difficult it is to remove an electron. Theref ...
Teacher Background Information: The periodic table is arranged in
... contain the same number of electrons but an increasing number of protons so the ionic radius decreases in size. The anions (P3-, S2- and Cl-) contain more electrons than protons and therefore are larger that the parent atom. Across a period, the ionic size decreases because the number of electrons r ...
... contain the same number of electrons but an increasing number of protons so the ionic radius decreases in size. The anions (P3-, S2- and Cl-) contain more electrons than protons and therefore are larger that the parent atom. Across a period, the ionic size decreases because the number of electrons r ...
unit iv – the periodic table
... electron cloud increases. That is, the atomic size increases as you go down the table. The reason for this is that you are adding energy levels as you go down the table (1, 2, 3,...). The positive charge of the nucleus increase as you go from left to right across the table. This increase in nuclear ...
... electron cloud increases. That is, the atomic size increases as you go down the table. The reason for this is that you are adding energy levels as you go down the table (1, 2, 3,...). The positive charge of the nucleus increase as you go from left to right across the table. This increase in nuclear ...
Chapter 5 The Periodic Table Section 1 Organizing the Elements
... and the transition metals. – alkali metal: one of the elements of Group 1 of the periodic table – alkaline-earth metal: one of the elements of Group 2 of the ...
... and the transition metals. – alkali metal: one of the elements of Group 1 of the periodic table – alkaline-earth metal: one of the elements of Group 2 of the ...
Introduction to Mendeleev*s Periodic Table of Elements
... • Be does not react with water. • Mg reacts with hot water. • Ca, Sr, Ba react easily with cold water. • Which way along the group does reactivity increase? ...
... • Be does not react with water. • Mg reacts with hot water. • Ca, Sr, Ba react easily with cold water. • Which way along the group does reactivity increase? ...
NAME - MrTestaScienceClass
... Graphing Periodic Trends Computer Activity – Academic Chemistry BACKGROUND: In 1870, Dmitri Mendeleev first proposed a new way of studying and organizing the then known 63 elements. The modern form of the table has been modified and improved many times since Mendeleev’s tables. Pioneers like Moseley ...
... Graphing Periodic Trends Computer Activity – Academic Chemistry BACKGROUND: In 1870, Dmitri Mendeleev first proposed a new way of studying and organizing the then known 63 elements. The modern form of the table has been modified and improved many times since Mendeleev’s tables. Pioneers like Moseley ...
Unit Two Test Review
... very low reactivity. good conductivity. very high reactivity. metallic character. ...
... very low reactivity. good conductivity. very high reactivity. metallic character. ...
Exam # 2 Review - HCC Learning Web
... • What is the maximum number of electrons that can occupy a p energy sublevel? • What is the maximum number of electrons that can occupy the 1st principal energy level? • What is the maximum number of electrons that can occupy the 2nd principal energy level? • Which electron sublevel follows the 4s ...
... • What is the maximum number of electrons that can occupy a p energy sublevel? • What is the maximum number of electrons that can occupy the 1st principal energy level? • What is the maximum number of electrons that can occupy the 2nd principal energy level? • Which electron sublevel follows the 4s ...
Alkaline Earth Metals
... • poor conductors of heat and electricity • in solid form, they are dull and brittle • usually have lower densities than metals • most of the crust, atmosphere and oceans are made up of nonmetals. • Bulk tissues of living organisms are composed almost entirely of nonmetals. • Many nonmetals (hydroge ...
... • poor conductors of heat and electricity • in solid form, they are dull and brittle • usually have lower densities than metals • most of the crust, atmosphere and oceans are made up of nonmetals. • Bulk tissues of living organisms are composed almost entirely of nonmetals. • Many nonmetals (hydroge ...
Lecture 10
... distance from the nucleus to a p electron is slightly larger than the average distance to an s electron in the same shell. There is a slight decrease from group 15 to group 16 due to electron-electron repulsion of electrons in the same orbital. ...
... distance from the nucleus to a p electron is slightly larger than the average distance to an s electron in the same shell. There is a slight decrease from group 15 to group 16 due to electron-electron repulsion of electrons in the same orbital. ...
Atomic radii decrease from left to right across a period
... metals to the noble gases; radii increase down each group (column). The radius increases sharply between the noble gasat the end of each period and the alkali metal at the beginning of the next period. These trends of the atomic radii (and of various other chemical and physical properties of the ele ...
... metals to the noble gases; radii increase down each group (column). The radius increases sharply between the noble gasat the end of each period and the alkali metal at the beginning of the next period. These trends of the atomic radii (and of various other chemical and physical properties of the ele ...
File
... The famous detective Sherlock Holmes used many kinds of clues to solve his cases. Like any good detective, he knew the value of fingerprints because no two people have the same fingerprints. In a way, atomic numbers are similar to fingerprints, because no two elements have the same atomic number. In ...
... The famous detective Sherlock Holmes used many kinds of clues to solve his cases. Like any good detective, he knew the value of fingerprints because no two people have the same fingerprints. In a way, atomic numbers are similar to fingerprints, because no two elements have the same atomic number. In ...
Periodic Trends Name: Part 1: Summary of the Periodic Trends
... b. How does this account for the trend you discovered in 1st ionization energy? ...
... b. How does this account for the trend you discovered in 1st ionization energy? ...
Chapter 7 The Development of the Periodic Table
... 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. ...
... 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. ...
History of the Periodic Table
... The familiar periodic table that adorns many science classrooms is based on a number of early efforts to identify and classify the elements. In the 1790’s, one of the first lists of elements and their compounds was compiled by French chemist Antioine-Laurent Lavioser. It was Lavoisier who divided th ...
... The familiar periodic table that adorns many science classrooms is based on a number of early efforts to identify and classify the elements. In the 1790’s, one of the first lists of elements and their compounds was compiled by French chemist Antioine-Laurent Lavioser. It was Lavoisier who divided th ...
Exam Essays
... The atomic number equals the number of protons in the nucleus of an atom and also equals the number of electrons in the neutral atom. The mass number is the sum of the number of protons and neutrons and can be used, with the atomic number, to find the number of neutrons in each isotope. Each isotope ...
... The atomic number equals the number of protons in the nucleus of an atom and also equals the number of electrons in the neutral atom. The mass number is the sum of the number of protons and neutrons and can be used, with the atomic number, to find the number of neutrons in each isotope. Each isotope ...
Chem.-Chapter-6-notes
... First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period. Cations are always smaller than the atoms from which they form. Anions are always larger than the atoms from which they form. In general, electronegativity values decrease fro ...
... First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period. Cations are always smaller than the atoms from which they form. Anions are always larger than the atoms from which they form. In general, electronegativity values decrease fro ...
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.