Chapter 6 The Periodic Table The how and why
... • Group number = number of electrons in highest energy level Transition metals- d orbitals Inner transition- f orbitals Noble gases s and p orbitals full ...
... • Group number = number of electrons in highest energy level Transition metals- d orbitals Inner transition- f orbitals Noble gases s and p orbitals full ...
Chapt6
... • Group number = number of electrons in highest energy level Transition metals- d orbitals Inner transition- f orbitals Noble gases s and p orbitals full ...
... • Group number = number of electrons in highest energy level Transition metals- d orbitals Inner transition- f orbitals Noble gases s and p orbitals full ...
PPTHANDOUTThe Modern Periodic Table
... alkaline; less _________________ than alkali or alkaline; for the most part their outermost electrons are in a d sublevel; exceptions to the electron configuration are found in these groups (Ex: Ni, Pd, ...
... alkaline; less _________________ than alkali or alkaline; for the most part their outermost electrons are in a d sublevel; exceptions to the electron configuration are found in these groups (Ex: Ni, Pd, ...
The Periodic Table
... In this graph we notice that the inert gases He, Ne and Ar all exhibit positive electron affinities. In other words forming He-1 is unfavorable relative to He. This makes sense since the inert gases have filled s and p levels (or filled octets if you prefer that terminology) and any additional elect ...
... In this graph we notice that the inert gases He, Ne and Ar all exhibit positive electron affinities. In other words forming He-1 is unfavorable relative to He. This makes sense since the inert gases have filled s and p levels (or filled octets if you prefer that terminology) and any additional elect ...
Microsoft Word - PeriodicTrends.doc
... The Periodic Table is arranged according to the Periodic Law. The Periodic Law states that when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern. These patterns can be discovered by examining the changes in properties of eleme ...
... The Periodic Table is arranged according to the Periodic Law. The Periodic Law states that when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern. These patterns can be discovered by examining the changes in properties of eleme ...
Graphing Trends in the Periodic Table
... number for Family IIA. 3. Make sure each scale is uniform and covers the range of numbers to be plotted. 4. Label the graph. Include a title and labels for each axis. Also include a key for the two lines. ...
... number for Family IIA. 3. Make sure each scale is uniform and covers the range of numbers to be plotted. 4. Label the graph. Include a title and labels for each axis. Also include a key for the two lines. ...
2. Classification of Elements and periodicity in properties
... ¾ These are monoatomic gases. ¾ They are chemically inactive. ¾ They are placed at the extreme right of the periodic table. REPRESENTATIVE ELEMENTS: ¾ s-block or p-block elements except '0' group are called representative elements. ¾ They have only one incomplete outer shell. ¾ These elements attain ...
... ¾ These are monoatomic gases. ¾ They are chemically inactive. ¾ They are placed at the extreme right of the periodic table. REPRESENTATIVE ELEMENTS: ¾ s-block or p-block elements except '0' group are called representative elements. ¾ They have only one incomplete outer shell. ¾ These elements attain ...
Oxidation Numbers, Begin Exam Review
... When F gains an electron it becomes an F-1 ion 1s2 2s2 2p5 becomes… 1s2 2s2 2p6 – 8 valence electrons F carries a -1 charge because it has gained an electron, and it now has more negatively charged electrons than positively charged protons ...
... When F gains an electron it becomes an F-1 ion 1s2 2s2 2p5 becomes… 1s2 2s2 2p6 – 8 valence electrons F carries a -1 charge because it has gained an electron, and it now has more negatively charged electrons than positively charged protons ...
Periodic Groups and Trends
... • Called alkali metals because they all react with water to form an alkali solution of the metal hydroxide and hydrogen gas. – i.e. Na(s) + H2O(l) NaOH(aq) + H2(g) ...
... • Called alkali metals because they all react with water to form an alkali solution of the metal hydroxide and hydrogen gas. – i.e. Na(s) + H2O(l) NaOH(aq) + H2(g) ...
Chapter 5 and 6 Notes Electromagnetic Radiation and Light Models
... • An ion is a positively or negatively charged atom that gains or loses an ___________________________. • A cation loses electrons and produces a _________________________ charge • An anion gains electrons and produces a _________________________ charge Ionic Radius - Cations • Groups 1A, 2A, 3A, an ...
... • An ion is a positively or negatively charged atom that gains or loses an ___________________________. • A cation loses electrons and produces a _________________________ charge • An anion gains electrons and produces a _________________________ charge Ionic Radius - Cations • Groups 1A, 2A, 3A, an ...
Chapter 5 and 6 Notes Electromagnetic Radiation and Light Models
... • An ion is a positively or negatively charged atom that gains or loses an ___________________________. • A cation loses electrons and produces a _________________________ charge • An anion gains electrons and produces a _________________________ charge Ionic Radius - Cations • Groups 1A, 2A, 3A, an ...
... • An ion is a positively or negatively charged atom that gains or loses an ___________________________. • A cation loses electrons and produces a _________________________ charge • An anion gains electrons and produces a _________________________ charge Ionic Radius - Cations • Groups 1A, 2A, 3A, an ...
CPO Science Link Teacher`s Guide
... where they would fall in the table. As new elements were discovered, his theory was proven correct. This table became the periodic table of elements. The periodic table organizes the elements according to how they combine with other elements due to their chemical properties. The elements are arrange ...
... where they would fall in the table. As new elements were discovered, his theory was proven correct. This table became the periodic table of elements. The periodic table organizes the elements according to how they combine with other elements due to their chemical properties. The elements are arrange ...
effective nuclear charge
... • The notion of Zeff explains this effect: For a manyelectron atom, the energies of orbitals with the same n value increase with increasing l value. – Ex) Carbon atom (1s22s22p2): The energy of the 2p orbital (l = 1) is higher than that of the 2s (l = 0) orbital. – This difference in energies is due ...
... • The notion of Zeff explains this effect: For a manyelectron atom, the energies of orbitals with the same n value increase with increasing l value. – Ex) Carbon atom (1s22s22p2): The energy of the 2p orbital (l = 1) is higher than that of the 2s (l = 0) orbital. – This difference in energies is due ...
Factors Affecting the Properties of Elements
... Since the distance from the nucleus to the outermost electrons increases due to the added orbits, the force of attraction between the nucleus and the valence electrons decreases, explaining these properties: atomic radius increases metallic character increases (elements have a weaker hold on ele ...
... Since the distance from the nucleus to the outermost electrons increases due to the added orbits, the force of attraction between the nucleus and the valence electrons decreases, explaining these properties: atomic radius increases metallic character increases (elements have a weaker hold on ele ...
Activity 2 Elements and Their Properties
... bodies different in form.” The first modern definition of element, which is not much different, is from Robert Boyle: “Bodies, which not being made of any other bodies, or of one another, are the ingredients of which all those . . . mixed bodies are . . . compounded.” Scientists now state that an el ...
... bodies different in form.” The first modern definition of element, which is not much different, is from Robert Boyle: “Bodies, which not being made of any other bodies, or of one another, are the ingredients of which all those . . . mixed bodies are . . . compounded.” Scientists now state that an el ...
Chapter 2 Atoms and Elements
... Isotopes are elements whose atoms differ in mass only. – They differ in mass because these elemental atoms have different number of neutrons. – They are the same element because they have the same number of protons (atomic number). – They are chemically identical. ...
... Isotopes are elements whose atoms differ in mass only. – They differ in mass because these elemental atoms have different number of neutrons. – They are the same element because they have the same number of protons (atomic number). – They are chemically identical. ...
tro2_ppt_lecture_02 - Louisiana Tech University
... Isotopes are elements whose atoms differ in mass only. – They differ in mass because these elemental atoms have different number of neutrons. – They are the same element because they have the same number of protons (atomic number). – They are chemically identical. ...
... Isotopes are elements whose atoms differ in mass only. – They differ in mass because these elemental atoms have different number of neutrons. – They are the same element because they have the same number of protons (atomic number). – They are chemically identical. ...
CHM1022 & CHM1639 Chemistry
... Hund’s rule states that when filling a set of orbitals at the same energy (sunshell), one electron is placed in each orbital before pairing occurs. Pauli’s principle tells us that when placing a second electron in an orbital, its spin must be opposite to the electron already in the orbital. (Spin is ...
... Hund’s rule states that when filling a set of orbitals at the same energy (sunshell), one electron is placed in each orbital before pairing occurs. Pauli’s principle tells us that when placing a second electron in an orbital, its spin must be opposite to the electron already in the orbital. (Spin is ...
January Exam Review
... C) The size of the atomic radius decreases as you move from left to right across a period. D) The size of the atomic radius increases and then decreases across a period. 4. The atomic size of an element is an example of a periodic property. The atomic size of the four elements below can be illustrat ...
... C) The size of the atomic radius decreases as you move from left to right across a period. D) The size of the atomic radius increases and then decreases across a period. 4. The atomic size of an element is an example of a periodic property. The atomic size of the four elements below can be illustrat ...
Standard
... The names of groups and periods on the periodic chart are alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. Metalloids have properties of metals and nonmetals. They are located between metals and nonmetals on the periodic table. Some are used in semiconductors. ...
... The names of groups and periods on the periodic chart are alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. Metalloids have properties of metals and nonmetals. They are located between metals and nonmetals on the periodic table. Some are used in semiconductors. ...
Chapter 4 notes
... Strategy Isoelectronic series are species with identical electron configurations but different nuclear charges. Determine the number of electrons in each species. The radii of isoelectronic series members decreases with increasing nuclear charge. Solution The isoelectronic series includes K+, Ar, P3 ...
... Strategy Isoelectronic series are species with identical electron configurations but different nuclear charges. Determine the number of electrons in each species. The radii of isoelectronic series members decreases with increasing nuclear charge. Solution The isoelectronic series includes K+, Ar, P3 ...
Agenda 11/4/2016
... - electrons are added to orbitals in the same principal energy level - Moving across a period the increased nuclear charge increases the attraction between the nucleus and the electrons in the orbitals in that energy level Therefore it is more difficult (takes more energy) to remove an electron from ...
... - electrons are added to orbitals in the same principal energy level - Moving across a period the increased nuclear charge increases the attraction between the nucleus and the electrons in the orbitals in that energy level Therefore it is more difficult (takes more energy) to remove an electron from ...
Document
... ● the number of outer shell electrons is the same; ● the number of complete electron shells increases by one. The number of a group is the same as the number of electrons in the outer shell of elements in that group, except for group 8. Trends across a period: ● the number of outer shell electrons i ...
... ● the number of outer shell electrons is the same; ● the number of complete electron shells increases by one. The number of a group is the same as the number of electrons in the outer shell of elements in that group, except for group 8. Trends across a period: ● the number of outer shell electrons i ...
Metals and Nonmetals Metals and Nonmetals
... – Includes the noble (inert) gases as a special case ...
... – Includes the noble (inert) gases as a special case ...
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.