Periodic Table and Trends 2013
... • All shells beneath the outermost have stable octet. – Except: Helium (He), Lithium (Li) & Beryllium (Be). First energy level is full with 2 electrons. ...
... • All shells beneath the outermost have stable octet. – Except: Helium (He), Lithium (Li) & Beryllium (Be). First energy level is full with 2 electrons. ...
Periodic Trends in Ionic Size
... Cations are smaller than the atoms from which they are formed. The loss of outer shell electrons results in increased attraction between the nucleus and the remaining electrons. This results in less electron-electron repulsion and allows the nucleus and the electrons to come closer together. When co ...
... Cations are smaller than the atoms from which they are formed. The loss of outer shell electrons results in increased attraction between the nucleus and the remaining electrons. This results in less electron-electron repulsion and allows the nucleus and the electrons to come closer together. When co ...
chapter5
... absorbed when an electron is added to an isolated gaseous atom to form an ion with a 1charge. • Sign conventions for electron affinity. – If electron affinity > 0 energy is absorbed. – If electron affinity < 0 energy is released. ...
... absorbed when an electron is added to an isolated gaseous atom to form an ion with a 1charge. • Sign conventions for electron affinity. – If electron affinity > 0 energy is absorbed. – If electron affinity < 0 energy is released. ...
CHAPTER 6
... absorbed when an electron is added to an isolated gaseous atom to form an ion with a 1charge. • Sign conventions for electron affinity. – If electron affinity > 0 energy is absorbed. – If electron affinity < 0 energy is released. ...
... absorbed when an electron is added to an isolated gaseous atom to form an ion with a 1charge. • Sign conventions for electron affinity. – If electron affinity > 0 energy is absorbed. – If electron affinity < 0 energy is released. ...
Chapter 2 - Department of Chemistry and Physics
... The atomic mass of an element on the periodic table is the weighted average of the masses of its stable isotopes For example H = 1.008 amu Calcium = 40.078 amu We will use these masses later for chemical calculations ...
... The atomic mass of an element on the periodic table is the weighted average of the masses of its stable isotopes For example H = 1.008 amu Calcium = 40.078 amu We will use these masses later for chemical calculations ...
CHAPTER 6
... • General periodic trend for electron affinity is – the values become more negative from left to right across a period on the periodic chart. – the values become more negative from bottom to top up a row on the periodic chart. ...
... • General periodic trend for electron affinity is – the values become more negative from left to right across a period on the periodic chart. – the values become more negative from bottom to top up a row on the periodic chart. ...
Group 17: The Halogens - Chemwiki
... it from hydrofluoric acid. Fluorine exists as a diatomic molecule in its free state (F2) and is the most abundant halogen found in the Earth's crust. Fluorine is the most electronegative element in the periodic table. It appears as a pale yellow gas at room temperature. Fluorine also has a relative ...
... it from hydrofluoric acid. Fluorine exists as a diatomic molecule in its free state (F2) and is the most abundant halogen found in the Earth's crust. Fluorine is the most electronegative element in the periodic table. It appears as a pale yellow gas at room temperature. Fluorine also has a relative ...
Atomic Radius
... The period trend in atomic radii has been correctly applied. Checking radii values in Figure 11 (slide 7) verifies the answer. Periodic Trends ...
... The period trend in atomic radii has been correctly applied. Checking radii values in Figure 11 (slide 7) verifies the answer. Periodic Trends ...
Trend #1 atomic mass
... There are 7 trends on the periodic table that we will follow. Using your periodic table, answer all of the questions in the packet. Think hard. The periodic table has _______ groups that go _____ + __________. The rows that go across left to right are called the _________________. Similar elements a ...
... There are 7 trends on the periodic table that we will follow. Using your periodic table, answer all of the questions in the packet. Think hard. The periodic table has _______ groups that go _____ + __________. The rows that go across left to right are called the _________________. Similar elements a ...
Periodic Trends
... radius chart, determine which of the elements in each pair has a larger atomic radius: 1. Cesium (Cs) and Potassium (K) 2. Calcium (Ca) and Gold (Au) 3. Rubidium (Rb) and Strontium (Sr) 4. Oxygen (O) and Sulfur (S) 5. Xenon (Xe) and Neon (Ne) 6. Aluminum (Al) and Tin (Sn) 7. Helium (He) and Fluorine ...
... radius chart, determine which of the elements in each pair has a larger atomic radius: 1. Cesium (Cs) and Potassium (K) 2. Calcium (Ca) and Gold (Au) 3. Rubidium (Rb) and Strontium (Sr) 4. Oxygen (O) and Sulfur (S) 5. Xenon (Xe) and Neon (Ne) 6. Aluminum (Al) and Tin (Sn) 7. Helium (He) and Fluorine ...
8th Grade Chap 4 Study Guide Answer Section
... 21. A material is said to be ductile if it a. is a mixture of a metal with at least one c. can be pulled out, or drawn, into a long other element. wire. b. can be hammered or rolled into flat sheets d. can transfer heat or electricity to another and other shapes. material. 22. The two most common al ...
... 21. A material is said to be ductile if it a. is a mixture of a metal with at least one c. can be pulled out, or drawn, into a long other element. wire. b. can be hammered or rolled into flat sheets d. can transfer heat or electricity to another and other shapes. material. 22. The two most common al ...
Chemistry Week 16
... Aufbau rule, Hund’s rule, and the Pauli exclusion principle that determine a probable location of an atom’s electrons. Students will go over the answers to the unit 5 test and rework the problems that they missed. ...
... Aufbau rule, Hund’s rule, and the Pauli exclusion principle that determine a probable location of an atom’s electrons. Students will go over the answers to the unit 5 test and rework the problems that they missed. ...
Slide 1
... • Mendeleev’s periodic table generally organized elements by increasing atomic mass and with similar properties in columns. In some places, there were missing elements whose properties he predicted. • When gallium, scandium, and germanium were isolated and characterized, their properties were almos ...
... • Mendeleev’s periodic table generally organized elements by increasing atomic mass and with similar properties in columns. In some places, there were missing elements whose properties he predicted. • When gallium, scandium, and germanium were isolated and characterized, their properties were almos ...
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN
... number. The modern periodic law given by Moseley is : “The properties of elements are periodic functions of their atomic numbers, i.e., if elements are arranged in the order of their atomic numbers. Similar elements are repeated after regular intervals”. He also gave the ...
... number. The modern periodic law given by Moseley is : “The properties of elements are periodic functions of their atomic numbers, i.e., if elements are arranged in the order of their atomic numbers. Similar elements are repeated after regular intervals”. He also gave the ...
Unit 2 - Electrons and Periodic Behavior
... 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. ...
Unit 3 Notes: Periodic Table Notes
... Most are radioactive and manmade Melting points vary, but usually higher than alkaline earth metals. Reactivity varies greatly Used for nuclear power/weapons, radiation therapy, fire alarms. Group 13: Boron Group Group 14: Carbon Group Group 15: Nitrogen Group Group 16: Oxygen Group Group 17 ...
... Most are radioactive and manmade Melting points vary, but usually higher than alkaline earth metals. Reactivity varies greatly Used for nuclear power/weapons, radiation therapy, fire alarms. Group 13: Boron Group Group 14: Carbon Group Group 15: Nitrogen Group Group 16: Oxygen Group Group 17 ...
Daily 40 no. – 15 John Newlands
... John Newlands was born in London in 1837 and died in 1898. He noticed that, when the elements are arranged in consecutive order of their atomic numbers, patterns emerge and thus proposed the Law of Octaves. He predicted the existence of germanium and studied at the Royal College of Chemistry. -Alann ...
... John Newlands was born in London in 1837 and died in 1898. He noticed that, when the elements are arranged in consecutive order of their atomic numbers, patterns emerge and thus proposed the Law of Octaves. He predicted the existence of germanium and studied at the Royal College of Chemistry. -Alann ...
Periodic Trends - MathewsClassroom
... The periodicity of properties of the elements is caused by the periodicity in electronic structure. The noble gases are chemically unreactive, or nearly so, because their electronic structures are stable--their atoms hold their quota of electrons strongly, have no affinity for more electrons, and ha ...
... The periodicity of properties of the elements is caused by the periodicity in electronic structure. The noble gases are chemically unreactive, or nearly so, because their electronic structures are stable--their atoms hold their quota of electrons strongly, have no affinity for more electrons, and ha ...
Lecture 1.9 PowerPoint
... • Elements that only need one (or two) electron to fill or “half” fill a subshell will have much higher electron affinities than element that already have a filled subshell. • Therefore, the only way to predict electron affinities is by examining the element’s electron configuration. • Electron affi ...
... • Elements that only need one (or two) electron to fill or “half” fill a subshell will have much higher electron affinities than element that already have a filled subshell. • Therefore, the only way to predict electron affinities is by examining the element’s electron configuration. • Electron affi ...
Periodic Trends - Chemwiki
... atomic radii. This distance is measured in picometers. Atomic radius patterns are observed throughout the periodic table. Atomic size gradually decreases from left to right across a period of elements. This is because, within a period or family of elements, all electrons are added to the same shell. ...
... atomic radii. This distance is measured in picometers. Atomic radius patterns are observed throughout the periodic table. Atomic size gradually decreases from left to right across a period of elements. This is because, within a period or family of elements, all electrons are added to the same shell. ...
Atomic Structure and the Periodic Table
... 6. The staircase line divides the metals, on the left, from the nonmentals, on the right. 7. a. The metalloids are located along the bold staircase. b. Examples of metalloids include aluminum and boron. c. A metalloid is an elements that has properties common to both metals and nonmetals. 8. As you ...
... 6. The staircase line divides the metals, on the left, from the nonmentals, on the right. 7. a. The metalloids are located along the bold staircase. b. Examples of metalloids include aluminum and boron. c. A metalloid is an elements that has properties common to both metals and nonmetals. 8. As you ...
2 Atoms, Bonding, and the Periodic Table
... the symbol for the element surrounded by dots that stand for valence electrons; Chemical bond: the force of attraction that holds two atoms together as a result of the rearrangement of electrons between them; Noble gas: any element in Group 18, which consists of elements with eight valence electrons ...
... the symbol for the element surrounded by dots that stand for valence electrons; Chemical bond: the force of attraction that holds two atoms together as a result of the rearrangement of electrons between them; Noble gas: any element in Group 18, which consists of elements with eight valence electrons ...
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.