CHEMICAL PERIODICITY
... • Good conductors of electricity and have a high luster • Less reactive than alkali and alkali-earth metal • Some (e.g. platinum and gold) are so unreactive that they do not form compounds easily. • Some are found as free element. ...
... • Good conductors of electricity and have a high luster • Less reactive than alkali and alkali-earth metal • Some (e.g. platinum and gold) are so unreactive that they do not form compounds easily. • Some are found as free element. ...
The Periodic Table
... • Some are like metals • Some are like non-metals • Properties vary greatly within a group ...
... • Some are like metals • Some are like non-metals • Properties vary greatly within a group ...
ionization energy
... Alkali Metal Reactions with O2 • Only lithium reacts with O2 to give the expected product, lithium oxide. 4Li(s) + O2(g) → 2Li2O(s) • Sodium reacts mainly to yield sodium peroxide. 2Na(s) + O2(g) → Na2O2(s) • Potassium reacts to yield mixtures of the oxide, peroxide, and superoxide. K(s) + O2(g) → ...
... Alkali Metal Reactions with O2 • Only lithium reacts with O2 to give the expected product, lithium oxide. 4Li(s) + O2(g) → 2Li2O(s) • Sodium reacts mainly to yield sodium peroxide. 2Na(s) + O2(g) → Na2O2(s) • Potassium reacts to yield mixtures of the oxide, peroxide, and superoxide. K(s) + O2(g) → ...
Chapter 8 PPT - Richsingiser.com
... Alkali Metal Reactions with O2 • Only lithium reacts with O2 to give the expected product, lithium oxide. 4Li(s) + O2(g) → 2Li2O(s) • Sodium reacts mainly to yield sodium peroxide. 2Na(s) + O2(g) → Na2O2(s) • Potassium reacts to yield mixtures of the oxide, peroxide, and superoxide. K(s) + O2(g) → ...
... Alkali Metal Reactions with O2 • Only lithium reacts with O2 to give the expected product, lithium oxide. 4Li(s) + O2(g) → 2Li2O(s) • Sodium reacts mainly to yield sodium peroxide. 2Na(s) + O2(g) → Na2O2(s) • Potassium reacts to yield mixtures of the oxide, peroxide, and superoxide. K(s) + O2(g) → ...
chemistry - Illini West High School
... electrons indicates the period on the periodic table in which it is found. • The number of valence electrons for elements in groups 13-18 is ten less than their group number. ...
... electrons indicates the period on the periodic table in which it is found. • The number of valence electrons for elements in groups 13-18 is ten less than their group number. ...
The Periodic Table
... metallic character. The scale is from Fr to F. Fr has the most metallic character and F has the least. In groups, metallic character increases with atomic number because each successive element gets closest to Fr. In periods, metallic character decreases when ...
... metallic character. The scale is from Fr to F. Fr has the most metallic character and F has the least. In groups, metallic character increases with atomic number because each successive element gets closest to Fr. In periods, metallic character decreases when ...
The periodic table and electron structure - Chemistry
... Na-8, Mg-9, Al-10, Si-11, P-12, S-13, Cl-14 and K-19, Ca-20, Ga-31, Ge-32, As-33, Se-34, Br-35 (Note that the third row would not have been completed by Newlands because a few of those elements were yet to be discovered such as gallium in 1875 and germanium in 1886. Bromine was a recent discovery in ...
... Na-8, Mg-9, Al-10, Si-11, P-12, S-13, Cl-14 and K-19, Ca-20, Ga-31, Ge-32, As-33, Se-34, Br-35 (Note that the third row would not have been completed by Newlands because a few of those elements were yet to be discovered such as gallium in 1875 and germanium in 1886. Bromine was a recent discovery in ...
atom - ealler
... The atoms of the each element emit a different light because they have their own electronic structure of the extra-nuclear part. 1. The atom consists of a small, positively-charged nucleus surrounded by electrons that travel in certain definite circular orbits or shells attracted by the nucleus. 2. ...
... The atoms of the each element emit a different light because they have their own electronic structure of the extra-nuclear part. 1. The atom consists of a small, positively-charged nucleus surrounded by electrons that travel in certain definite circular orbits or shells attracted by the nucleus. 2. ...
Unit #1 Review – Answers Chapter 1 Review – p. 62 #1, 4
... 20. Describe the trends in the periodic table for each of the following atomic properties, and give a theoretical explanation for each trend: a) Atomic radii decrease as you move from left to right across each period. From left to right across a period, the nuclear charge increases while the shieldi ...
... 20. Describe the trends in the periodic table for each of the following atomic properties, and give a theoretical explanation for each trend: a) Atomic radii decrease as you move from left to right across each period. From left to right across a period, the nuclear charge increases while the shieldi ...
The Periodic Table
... Why are Noble Gases so unreactive? They contain a full octet – atoms gain/lose electrons to achieve noble gas notation ...
... Why are Noble Gases so unreactive? They contain a full octet – atoms gain/lose electrons to achieve noble gas notation ...
Essentials of Biology Sylvia S. Mader
... Arrangements of Electrons in an Atom • Electrons encircle the nucleus of an atom at discrete energy levels called electron shells. • In atoms with two or more shells, the outer shell follows the octet rule (8 electrons) • The electrons in the outer valence shell determine the chemical reactivity of ...
... Arrangements of Electrons in an Atom • Electrons encircle the nucleus of an atom at discrete energy levels called electron shells. • In atoms with two or more shells, the outer shell follows the octet rule (8 electrons) • The electrons in the outer valence shell determine the chemical reactivity of ...
Periodic Trends
... Energy needed to remove an electron from an atom or molecule. The higher the effective core charge and lower the number of electrons shells, the greater the ionization energy How big (e.g., radius) an atom is Atomic radius is measured from the center of the nucleus to the valence electron shell. The ...
... Energy needed to remove an electron from an atom or molecule. The higher the effective core charge and lower the number of electrons shells, the greater the ionization energy How big (e.g., radius) an atom is Atomic radius is measured from the center of the nucleus to the valence electron shell. The ...
Chapter 5
... discovered that the elements fit into patterns better when they were arranged according to atomic number, rather than atomic weight. • The Periodic Law states that the physical and chemical properties of the elements are periodic functions of their atomic numbers. ...
... discovered that the elements fit into patterns better when they were arranged according to atomic number, rather than atomic weight. • The Periodic Law states that the physical and chemical properties of the elements are periodic functions of their atomic numbers. ...
Atoms
... because of increasing Z*. -radii increase down a group because of the increasing distance of the electrons from the nucleus. - increasing distance from the nucleus outweighs effective nuclear charge for atomic radii down a group. ...
... because of increasing Z*. -radii increase down a group because of the increasing distance of the electrons from the nucleus. - increasing distance from the nucleus outweighs effective nuclear charge for atomic radii down a group. ...
Periods and Blocks of the Periodic Table
... • In many compounds, the negative charge of the valence electrons is concentrated closer to one atom than to another. • Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound. • Electronegativities tend to increase acros ...
... • In many compounds, the negative charge of the valence electrons is concentrated closer to one atom than to another. • Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound. • Electronegativities tend to increase acros ...
Periodic Trends - Chemwiki
... Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase. Conceptually, ionization energy is the opposite of electronegativity. The lower this energy is, the more readily the atom becomes a cation. Therefore, the higher this energy is, the more unlikel ...
... Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase. Conceptually, ionization energy is the opposite of electronegativity. The lower this energy is, the more readily the atom becomes a cation. Therefore, the higher this energy is, the more unlikel ...
Chem Activity: Polyatomic Ions
... 2. Take out a Periodic Table. Refer to it as you investigate group and period properties. Model Set 1: Atomic Radius 1. Use a textbook to find the definition of atomic radius and write the definition below. ...
... 2. Take out a Periodic Table. Refer to it as you investigate group and period properties. Model Set 1: Atomic Radius 1. Use a textbook to find the definition of atomic radius and write the definition below. ...
The Periodic Table - Journigan-wiki
... Metals - Low ionization energy Nonmetals - High ionization energy ...
... Metals - Low ionization energy Nonmetals - High ionization energy ...
Unit 3.pmd
... 39. Explain the following: (a) Electronegativity of elements increase on moving from left to right in the periodic table. (b) Ionisation enthalpy decrease in a group from top to bottom? 40. How does the metallic and non metallic character vary on moving from left to right in a period? 41. The radiu ...
... 39. Explain the following: (a) Electronegativity of elements increase on moving from left to right in the periodic table. (b) Ionisation enthalpy decrease in a group from top to bottom? 40. How does the metallic and non metallic character vary on moving from left to right in a period? 41. The radiu ...
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 ...
Periodic Classification of Element (NCERT )
... On moving down a group, ionization enthalpy generally decreases due to an increase in the atomic size and shielding. Thus, on moving down group 13, ionization enthalpy decreases from B to Al. But, Ga has higher ionization enthalpy than Al. Al follows mmediately after s–block elements, whereas Ga fol ...
... On moving down a group, ionization enthalpy generally decreases due to an increase in the atomic size and shielding. Thus, on moving down group 13, ionization enthalpy decreases from B to Al. But, Ga has higher ionization enthalpy than Al. Al follows mmediately after s–block elements, whereas Ga fol ...
The Periodic Table Test Review (3a-3b)
... 16. Identify the representative elements from the list given below. Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge 17. Why is argon placed before potassium in the modern periodic table? 18. Why do elements in the same group have similar properties? 19. Why is the size of a sodium ion (Na+) less than that of ...
... 16. Identify the representative elements from the list given below. Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge 17. Why is argon placed before potassium in the modern periodic table? 18. Why do elements in the same group have similar properties? 19. Why is the size of a sodium ion (Na+) less than that of ...
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.