Chapter 6 Review Name Period _____ Know the history
... They contain the same number of valence electrons 18. Where, generally, are the metals located on the periodic table? To the left of the staircase 19. Where, generally, are the nonmetals located on the periodic table? To the right of the staircase 20. List some properties of metals. High luster, duc ...
... They contain the same number of valence electrons 18. Where, generally, are the metals located on the periodic table? To the left of the staircase 19. Where, generally, are the nonmetals located on the periodic table? To the right of the staircase 20. List some properties of metals. High luster, duc ...
Chapter 5
... the number of protons in the nucleus. Atomic number (protons) was more important than atomic mass (protons+neutrons) ...
... the number of protons in the nucleus. Atomic number (protons) was more important than atomic mass (protons+neutrons) ...
The Periodic Table - Duplin County Schools
... Atomic Symbol: The atomic symbol is one or two letters chosen to represent an element ("H" for "hydrogen," etc.). These symbols are used every where in the world Usually, a symbol is the abbreviation of the element or the abbreviated Latin name of the element. ...
... Atomic Symbol: The atomic symbol is one or two letters chosen to represent an element ("H" for "hydrogen," etc.). These symbols are used every where in the world Usually, a symbol is the abbreviation of the element or the abbreviated Latin name of the element. ...
Name Date ______ Period ______ Chapter 5: Periodic Table
... 9. Nonmetals that are solids at room temperature tend to be brittle. If they are hit with a hammer, they shatter, or crumble. 10. ___________________________________ are located on the periodic table between metals and nonmetals. 11. _____________are elements with properties that fall between those ...
... 9. Nonmetals that are solids at room temperature tend to be brittle. If they are hit with a hammer, they shatter, or crumble. 10. ___________________________________ are located on the periodic table between metals and nonmetals. 11. _____________are elements with properties that fall between those ...
chapter-8- alklimetal
... – Prepared by electrolysis of chloride salts – Strong bases – Highly soluble in water ...
... – Prepared by electrolysis of chloride salts – Strong bases – Highly soluble in water ...
The Periodic Table
... from top to bottom down a group. • This is due to the increasing distance the electrons are from the nucleus. Each time a new principle energy level (shell) is added the orbiting electrons are at a higher energy and are further away from the nucleus. ...
... from top to bottom down a group. • This is due to the increasing distance the electrons are from the nucleus. Each time a new principle energy level (shell) is added the orbiting electrons are at a higher energy and are further away from the nucleus. ...
Instructional-Objectives
... Describe the basic properties of protons, neutrons, and electrons. 3.2 Atomic Number and Mass Number 3.2 Describe and define atomic and mass numbers Calculate the number of protons, neutrons, and electrons in any atom. Distinguish among atoms, ions, and isotopes. 3.3 Isotopes and Atomic Masses ...
... Describe the basic properties of protons, neutrons, and electrons. 3.2 Atomic Number and Mass Number 3.2 Describe and define atomic and mass numbers Calculate the number of protons, neutrons, and electrons in any atom. Distinguish among atoms, ions, and isotopes. 3.3 Isotopes and Atomic Masses ...
Instructional Objectives 3. Atomic Structure and the Periodic Table
... • Describe the basic properties of protons, neutrons, and electrons. 3.2 Atomic Number and Mass Number 3.2 Describe and define atomic and mass numbers • Calculate the number of protons, neutrons, and electrons in any atom. • Distinguish among atoms, ions, and isotopes. 3.3 Isotopes and Atomic Mass ...
... • Describe the basic properties of protons, neutrons, and electrons. 3.2 Atomic Number and Mass Number 3.2 Describe and define atomic and mass numbers • Calculate the number of protons, neutrons, and electrons in any atom. • Distinguish among atoms, ions, and isotopes. 3.3 Isotopes and Atomic Mass ...
File
... the nearly empty outer electron shells of the typical metals and the nearly filled electron shells of the nonmetals. Most of these elements are important industrial materials, being used to make transistors and other semiconductor devices, ceramics, solar batteries, and certain polymers. Metalloids ...
... the nearly empty outer electron shells of the typical metals and the nearly filled electron shells of the nonmetals. Most of these elements are important industrial materials, being used to make transistors and other semiconductor devices, ceramics, solar batteries, and certain polymers. Metalloids ...
Periodic Table
... One loosely bound valence electron Largest atomic radii in their periods Low ionization energies Low electronegativities ...
... One loosely bound valence electron Largest atomic radii in their periods Low ionization energies Low electronegativities ...
Hist PeriodicTable 2014
... • The elements in the same period have the same number of valence shells. (outermost path of an electron) ...
... • The elements in the same period have the same number of valence shells. (outermost path of an electron) ...
Hist PeriodicTable 2014
... • The elements in the same period have the same number of valence shells. (outermost path of an electron) ...
... • The elements in the same period have the same number of valence shells. (outermost path of an electron) ...
Unit 2 Materials NEW CONCEPTS/STANDARDS
... 8. Determine properties of elements by the number and arrangement of the electrons in the atom. 9. Calculate the number of protons, neutrons, and electrons in isotopes of an element. 10. Understand that ionic solids are held together by electrostatic attractions. 11. Convert from Celsius to Kelvin t ...
... 8. Determine properties of elements by the number and arrangement of the electrons in the atom. 9. Calculate the number of protons, neutrons, and electrons in isotopes of an element. 10. Understand that ionic solids are held together by electrostatic attractions. 11. Convert from Celsius to Kelvin t ...
The Periodic Table
... By doing this he saw fewer irregularities Moseley’s periodic table is what is used today. ...
... By doing this he saw fewer irregularities Moseley’s periodic table is what is used today. ...
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 ...
File - Lenora Henderson`s Flipped Chemistry Classroom
... Reading the Periodic Table Key Question What information can be displayed in a periodic table? The symbols and names of the elements, along with information about the structure of their atoms. Group 1A elements are called alkali metals Group 2A elements are called alkaline-earth metals Group ...
... Reading the Periodic Table Key Question What information can be displayed in a periodic table? The symbols and names of the elements, along with information about the structure of their atoms. Group 1A elements are called alkali metals Group 2A elements are called alkaline-earth metals Group ...
Revision map for the Periodic Table
... 1. The Periodic Table is a way of arranging what we know about the chemical elements. 2. Each element in the Periodic Table is a different type of atom. 3. Each element has a different atomic number. 4. The Periodic Table is arranged in atomic number order. 5. Each atom has an atomic number. 6. An e ...
... 1. The Periodic Table is a way of arranging what we know about the chemical elements. 2. Each element in the Periodic Table is a different type of atom. 3. Each element has a different atomic number. 4. The Periodic Table is arranged in atomic number order. 5. Each atom has an atomic number. 6. An e ...
Chemistry Ch. 5
... The atomic number refers to how many protons or electrons an atom of that element has. For instance, hydrogen has 1 proton, so it’s atomic number is 1. The atomic number is unique to that element. No two elements have the same atomic number. ...
... The atomic number refers to how many protons or electrons an atom of that element has. For instance, hydrogen has 1 proton, so it’s atomic number is 1. The atomic number is unique to that element. No two elements have the same atomic number. ...
5.1 Review and KEY
... Mendeleev noticed that certain similarities in the chemical properties of elements appeared at regular intervals when the elements were arranged in order of increasing (a) density. (b) reactivity. ...
... Mendeleev noticed that certain similarities in the chemical properties of elements appeared at regular intervals when the elements were arranged in order of increasing (a) density. (b) reactivity. ...
The Periodic Table
... 5. The nobel gases are found in group 18. Their outer energy level is filled, and they are very nonreactive, colorless gases. Shade the nobel gases red. 6. Halogens have seven electrons in the outer shell. They are located in group 17 on the periodic table. Halogens react with metals to form salts. ...
... 5. The nobel gases are found in group 18. Their outer energy level is filled, and they are very nonreactive, colorless gases. Shade the nobel gases red. 6. Halogens have seven electrons in the outer shell. They are located in group 17 on the periodic table. Halogens react with metals to form salts. ...
The Periodic Table
... Describe the Periodic Table Elements have different atomic masses - the number of protons plus neutrons increases up the table. • Rows - elements of each row have the same number of energy levels (shells). • Columns - elements have the same number of electrons in the outermost energy level or shell ...
... Describe the Periodic Table Elements have different atomic masses - the number of protons plus neutrons increases up the table. • Rows - elements of each row have the same number of energy levels (shells). • Columns - elements have the same number of electrons in the outermost energy level or shell ...
Describe the Periodic Table
... Atomic Symbol: 0The atomic symbol is one or two letters chosen to represent an element ("H" for "hydrogen," etc.). 0 These symbols are used every where in the world 0 Usually, a symbol is the abbreviation of the element or the abbreviated Latin name of the element. ...
... Atomic Symbol: 0The atomic symbol is one or two letters chosen to represent an element ("H" for "hydrogen," etc.). 0 These symbols are used every where in the world 0 Usually, a symbol is the abbreviation of the element or the abbreviated Latin name of the element. ...
Periodic Table
... Periodic Table Matching Match each item with the correct statement below. a. electronegativity f. b. ionization energy g. c. atomic radius h. d. metal i. e. transition metal j. ____ ____ ____ ____ ____ ...
... Periodic Table Matching Match each item with the correct statement below. a. electronegativity f. b. ionization energy g. c. atomic radius h. d. metal i. e. transition metal j. ____ ____ ____ ____ ____ ...
Page 1
... 1s22s22p63s23p64s23d104p65s2 Eighteen Elements tend to react in such a way as to attain the electron configuration of the atoms of the noble gas nearest to them in the Periodic Table. sodium ion chloride S21s22s22p63s23p6 bottom left The ion will be much smaller. In forming the ion, the atom loses a ...
... 1s22s22p63s23p64s23d104p65s2 Eighteen Elements tend to react in such a way as to attain the electron configuration of the atoms of the noble gas nearest to them in the Periodic Table. sodium ion chloride S21s22s22p63s23p6 bottom left The ion will be much smaller. In forming the ion, the atom loses a ...
Chapter 4
... 38 different elements, he found that the wavelengths of the lines in the spectra decreased in a regular manner as ______________ _________ increased. When the elements were arranged by increasing ____________ __________, the discrepancies in Mendeleev’s table disappeared. Mendeleev’s principle of ch ...
... 38 different elements, he found that the wavelengths of the lines in the spectra decreased in a regular manner as ______________ _________ increased. When the elements were arranged by increasing ____________ __________, the discrepancies in Mendeleev’s table disappeared. Mendeleev’s principle of ch ...
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.