The Periodic Table of the Elements
... The physical and chemical properties of the elements are periodic functions of their atomic numbers. In other words, when the elements are arranged in order of increasing atomic number, elements with similar properties appear at regular intervals. ...
... The physical and chemical properties of the elements are periodic functions of their atomic numbers. In other words, when the elements are arranged in order of increasing atomic number, elements with similar properties appear at regular intervals. ...
Chapter 6 the periodic table
... which they form. Anions are always larger than the atom from which they form. ...
... which they form. Anions are always larger than the atom from which they form. ...
Chapter 13
... the outermost s and p sublevels are filled Also called inert gases because they do not react with other elements – they are stable on their own Helium has 2 valence electrons (full 1s sublevel) The rest of the noble gases have 8 valence electrons (full s and p sublevels): Ne, Ar, Kr, Xe, Rn ...
... the outermost s and p sublevels are filled Also called inert gases because they do not react with other elements – they are stable on their own Helium has 2 valence electrons (full 1s sublevel) The rest of the noble gases have 8 valence electrons (full s and p sublevels): Ne, Ar, Kr, Xe, Rn ...
October 11, 2007
... 20th century chemistry has shown that these groups have similar electronic configurations This demonstrating that the behavior of the elements is a consequence of the number and configuration of their electrons only: only The atomic nucleus is unimportant chemically The electrons that are the most ...
... 20th century chemistry has shown that these groups have similar electronic configurations This demonstrating that the behavior of the elements is a consequence of the number and configuration of their electrons only: only The atomic nucleus is unimportant chemically The electrons that are the most ...
ch3 - sscyr11chemistry
... From Question 27 we know that 10 g of calcium requires 4 g of oxygen to convert it to calcium oxide. Therefore, if 10 g of oxygen is reacted with calcium until all of the calcium has reacted, there would be 6 g of oxygen remaining. Heinemann Chemistry 1 (4th edition) Reed International Books Austr ...
... From Question 27 we know that 10 g of calcium requires 4 g of oxygen to convert it to calcium oxide. Therefore, if 10 g of oxygen is reacted with calcium until all of the calcium has reacted, there would be 6 g of oxygen remaining. Heinemann Chemistry 1 (4th edition) Reed International Books Austr ...
ch3 - ChemistryVCE
... From Question 27 we know that 10 g of calcium requires 4 g of oxygen to convert it to calcium oxide. Therefore, if 10 g of oxygen is reacted with calcium until all of the calcium has reacted, there would be 6 g of oxygen remaining. Heinemann Chemistry 1 (4th edition) Reed International Books Austr ...
... From Question 27 we know that 10 g of calcium requires 4 g of oxygen to convert it to calcium oxide. Therefore, if 10 g of oxygen is reacted with calcium until all of the calcium has reacted, there would be 6 g of oxygen remaining. Heinemann Chemistry 1 (4th edition) Reed International Books Austr ...
Cations (positive ions) are smaller than their respective atoms.
... Is defined as the energy required to remove an electron from an atom in the gas phase. Each atom can have a series of ionization energies, since more than one electron can always be removed ...
... Is defined as the energy required to remove an electron from an atom in the gas phase. Each atom can have a series of ionization energies, since more than one electron can always be removed ...
Chapter 5: Electrons
... attracts electrons in the same energy level. Therefore, it is tougher to remove an electron from an atom. Increasing nuclear charge is responsible for both an increasing ionization energy and decreasing atomic radius across a period. ...
... attracts electrons in the same energy level. Therefore, it is tougher to remove an electron from an atom. Increasing nuclear charge is responsible for both an increasing ionization energy and decreasing atomic radius across a period. ...
Midterm Review
... Write the FULL electron configurations and orbital diagram/notation for each of the following ...
... Write the FULL electron configurations and orbital diagram/notation for each of the following ...
Midterm Review
... Write the FULL electron configurations and orbital diagram/notation for each of the following ...
... Write the FULL electron configurations and orbital diagram/notation for each of the following ...
The Periodic Table
... React readily with Group 6 React readily with water (though not as rapidly as the alkali metals) Two valence electron so they want to lose 2 electrons and achieve a noble configuration (an octet) form +2 cations ...
... React readily with Group 6 React readily with water (though not as rapidly as the alkali metals) Two valence electron so they want to lose 2 electrons and achieve a noble configuration (an octet) form +2 cations ...
The Periodic Table
... • Although elements in the same group have the same number of electrons in their outer shells, the atoms become larger as you move down and this also effects the properties of the elements. • We can look at the properties of elements in two ways: – The properties that relate to individual atoms of t ...
... • Although elements in the same group have the same number of electrons in their outer shells, the atoms become larger as you move down and this also effects the properties of the elements. • We can look at the properties of elements in two ways: – The properties that relate to individual atoms of t ...
Periodic Classification of Elements
... Question 5: Besides gallium, which other elements have since been discovered that were left by Mendeleev in his Periodic Table? (any two) Answer: Scandium and germanium Question 6: What were the criteria used by Mendeleev in creating his Periodic Table? Answer: Mendeleev’s periodic table was based o ...
... Question 5: Besides gallium, which other elements have since been discovered that were left by Mendeleev in his Periodic Table? (any two) Answer: Scandium and germanium Question 6: What were the criteria used by Mendeleev in creating his Periodic Table? Answer: Mendeleev’s periodic table was based o ...
Chapter 2 ATOMS AND ELEMENTS
... • This tells us the mass of one atom of an element relative to one atom of another element. • OR — the mass of 1000 atoms of one relative to 1000 atoms of another. • For example, an O atom is approximately 16 times heavier than an H atom. • Define one element as the standard against which all others ...
... • This tells us the mass of one atom of an element relative to one atom of another element. • OR — the mass of 1000 atoms of one relative to 1000 atoms of another. • For example, an O atom is approximately 16 times heavier than an H atom. • Define one element as the standard against which all others ...
Document
... 1. Graph on graph paper, the trend of first ionization energy (potential). The graph should have the atomic number on the x-axis and ionization energy on the y-axis. Label element symbols at the peaks and valleys. 2. Answer the questions below about this graph and what conclusions you would draw. Qu ...
... 1. Graph on graph paper, the trend of first ionization energy (potential). The graph should have the atomic number on the x-axis and ionization energy on the y-axis. Label element symbols at the peaks and valleys. 2. Answer the questions below about this graph and what conclusions you would draw. Qu ...
Periodic Table - Doral Academy Preparatory
... 2. What is the periodic law, and how can it be used to predict physical and chemical properties of elements? 3. What is the overall organization of the modern Periodic Table? 1. Three types of elements 2. Named groups ...
... 2. What is the periodic law, and how can it be used to predict physical and chemical properties of elements? 3. What is the overall organization of the modern Periodic Table? 1. Three types of elements 2. Named groups ...
Periodic Table - Doral Academy Preparatory
... 2. What is the periodic law, and how can it be used to predict physical and chemical properties of elements? 3. What is the overall organization of the modern Periodic Table? 1. Three types of elements 2. Named groups ...
... 2. What is the periodic law, and how can it be used to predict physical and chemical properties of elements? 3. What is the overall organization of the modern Periodic Table? 1. Three types of elements 2. Named groups ...
Chapter 5: The Periodic Law
... forming a positive ion first ionization energy: energy required to remove the first outermost electron ...
... forming a positive ion first ionization energy: energy required to remove the first outermost electron ...
The Periodic Table - Anderson High School
... Groups…Here’s Where the Periodic Table Gets Useful!! • Elements in the same group have similar chemical and physical properties!! (Mendeleev did that on purpose.) • Elements in the”A” groups are called representative elements. ...
... Groups…Here’s Where the Periodic Table Gets Useful!! • Elements in the same group have similar chemical and physical properties!! (Mendeleev did that on purpose.) • Elements in the”A” groups are called representative elements. ...
The Periodic Table
... Groups…Here’s Where the Periodic Table Gets Useful!! • Elements in the same group have similar chemical and physical properties!! (Mendeleev did that on purpose.) • Elements in the”A” groups are called representative elements. ...
... Groups…Here’s Where the Periodic Table Gets Useful!! • Elements in the same group have similar chemical and physical properties!! (Mendeleev did that on purpose.) • Elements in the”A” groups are called representative elements. ...
are smaller than their respective atoms.
... Is defined as the energy required to remove an electron from an atom in the gas phase. Each atom can have a series of ionization energies, since more than one electron can always be removed ...
... Is defined as the energy required to remove an electron from an atom in the gas phase. Each atom can have a series of ionization energies, since more than one electron can always be removed ...
Unit 3.pmd
... electron repulsion outweighs the stability gained by achieving noble gas configuration. ...
... electron repulsion outweighs the stability gained by achieving noble gas configuration. ...
to chapter:3
... complete basis for the periodic table. In that same year Englishman Cockroft and the Irishman Walton first split an atom by bombarding lithium in a particle accelerator, changing it to two helium nuclei. In 1945 Glenn Seaborg identified lanthanides and actinides (atomic number >92), which are usuall ...
... complete basis for the periodic table. In that same year Englishman Cockroft and the Irishman Walton first split an atom by bombarding lithium in a particle accelerator, changing it to two helium nuclei. In 1945 Glenn Seaborg identified lanthanides and actinides (atomic number >92), which are usuall ...
The Periodic Table - TangHua2012-2013
... from the left to the right across a period • Group - reactivity decreases as you go down the group. • Why? The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electrons. ...
... from the left to the right across a period • Group - reactivity decreases as you go down the group. • Why? The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electrons. ...
Exam Essays
... Elements fill the 4s sublevel with electrons before filling the 3d sublevels because the 4s sublevel is lower in energy than the 3d sublevels. According to the Aufbau principle, an electron occupies the lowest energy level that can receive it. Some elements move an electron from a filled 4s sublevel ...
... Elements fill the 4s sublevel with electrons before filling the 3d sublevels because the 4s sublevel is lower in energy than the 3d sublevels. According to the Aufbau principle, an electron occupies the lowest energy level that can receive it. Some elements move an electron from a filled 4s sublevel ...
Group 3 element
Group 3 is a group of elements in the periodic table. This group, like other d-block groups, should contain four elements, but it is not agreed what elements belong in the group. Scandium (Sc) and yttrium (Y) are always included, but the other two spaces are usually occupied by lanthanum (La) and actinium (Ac), or by lutetium (Lu) and lawrencium (Lr); less frequently, it is considered the group should be expanded to 32 elements (with all the lanthanides and actinides included) or contracted to contain only scandium and yttrium. The group itself has not acquired a trivial name; however, scandium, yttrium and the lanthanides are sometimes called rare earth metals.Three group 3 elements occur naturally, scandium, yttrium, and either lanthanum or lutetium. Lanthanum continues the trend started by two lighter members in general chemical behavior, while lutetium behaves more similarly to yttrium. This is in accordance with the trend for period 6 transition metals to behave more similarly to their upper periodic table neighbors. This trend is seen from hafnium, which is almost identical chemically to zirconium, to mercury, which is quite distant chemically from cadmium, but still shares with it almost equal atomic size and other similar properties. They all are silvery-white metals under standard conditions. The fourth element, either actinium or lawrencium, has only radioactive isotopes. Actinium, which occurs only in trace amounts, continues the trend in chemical behavior for metals that form tripositive ions with a noble gas configuration; synthetic lawrencium is calculated and partially shown to be more similar to lutetium and yttrium. So far, no experiments have been conducted to synthesize any element that could be the next group 3 element. Unbiunium (Ubu), which could be considered a group 3 element if preceded by lanthanum and actinium, might be synthesized in the near future, it being only three spaces away from the current heaviest element known, ununoctium.