Topic 5 - Holy Cross Collegiate
... Mendeleev had noticed a periodic relationship between increasing atomic mass and chemical properties of elements. His work provided a logical organization for a huge amount of data about the elements, but no one could explain why the elements showed their amazing periodicity. By about 1915, chemists ...
... Mendeleev had noticed a periodic relationship between increasing atomic mass and chemical properties of elements. His work provided a logical organization for a huge amount of data about the elements, but no one could explain why the elements showed their amazing periodicity. By about 1915, chemists ...
Periodic Table and Trends
... The top, right-area of the periodic table has the smallest atomic radius (Fluorine) Which would you assume to have the largest atomic radius: Al, Al+, or AlWhich would you assume to have the smallest atomic radius: C2+, C+, C, C-, C2- ...
... The top, right-area of the periodic table has the smallest atomic radius (Fluorine) Which would you assume to have the largest atomic radius: Al, Al+, or AlWhich would you assume to have the smallest atomic radius: C2+, C+, C, C-, C2- ...
Station 1: The Periodic Table 1a. Students know how to relate the
... How are groups identified? o Groups can be identified in two different ways. By number and name. Group 1 is also known as the Alkali Metals (except H). Group 2 is known as the Alkaline Earth Metals. Group 17 is known as the Halogens. Group 18 is known as the Noble Gases. o Elements that ...
... How are groups identified? o Groups can be identified in two different ways. By number and name. Group 1 is also known as the Alkali Metals (except H). Group 2 is known as the Alkaline Earth Metals. Group 17 is known as the Halogens. Group 18 is known as the Noble Gases. o Elements that ...
the periodic law
... 7. Period trends – ionization energies of main group elements increase across each period a. Slight increase between IIA and IIIA due to p-sublevels having a higher energy so electrons are easier to remove b. Slight decrease between VA and VIA due to paired electrons in the p-sublevel. Paired e- ha ...
... 7. Period trends – ionization energies of main group elements increase across each period a. Slight increase between IIA and IIIA due to p-sublevels having a higher energy so electrons are easier to remove b. Slight decrease between VA and VIA due to paired electrons in the p-sublevel. Paired e- ha ...
reviewing key trends
... 9. Using the graph on the attached sheet labeled “Periodicity of Atomic Radius”: a) Circle the points corresponding to the peaks on the graph. Write the symbol for the element at each peak. b) Put a square around the points corresponding to the troughs on the graph. Write the symbol for the element ...
... 9. Using the graph on the attached sheet labeled “Periodicity of Atomic Radius”: a) Circle the points corresponding to the peaks on the graph. Write the symbol for the element at each peak. b) Put a square around the points corresponding to the troughs on the graph. Write the symbol for the element ...
How to 2 Video Narrative
... Periods are horizontal rows on the Periodic Table. Periods go across the Periodic Table from the left to the right. Recall the location of the atomic numbers of the elements. Do you notice how the atomic numbers increase as you move left to right—or horizontally—in a period? The first row is called ...
... Periods are horizontal rows on the Periodic Table. Periods go across the Periodic Table from the left to the right. Recall the location of the atomic numbers of the elements. Do you notice how the atomic numbers increase as you move left to right—or horizontally—in a period? The first row is called ...
Chemistry 1 Notes #10 Chapter 6 Modern Periodic Table
... • lithium, sodium, potassium, rubidium, cesium, and francium • In their pure state, all of the alkali metals have a silvery appearance and are soft enough to cut with a knife. ...
... • lithium, sodium, potassium, rubidium, cesium, and francium • In their pure state, all of the alkali metals have a silvery appearance and are soft enough to cut with a knife. ...
Chem 115 POGIL Worksheet
... based on atomic number, became possible in 1913, when Henry G. J. Moseley found that the atomic numbers of elements could be determined experimentally from their characteristic x-ray frequencies. Today the periodic law is based on atomic numbers, rather than atomic weights: The properties of element ...
... based on atomic number, became possible in 1913, when Henry G. J. Moseley found that the atomic numbers of elements could be determined experimentally from their characteristic x-ray frequencies. Today the periodic law is based on atomic numbers, rather than atomic weights: The properties of element ...
Unit 13
... A Little Bit of History C In the early 1800s, German chemist J.W. Dobereiner observed that several elements could be classified into sets of three which he called triads. C (Li, Na, K), (Ca, Sr, Ba), (Cl, Br, I) C The elements within each triad had similar properties. C Several physical properties o ...
... A Little Bit of History C In the early 1800s, German chemist J.W. Dobereiner observed that several elements could be classified into sets of three which he called triads. C (Li, Na, K), (Ca, Sr, Ba), (Cl, Br, I) C The elements within each triad had similar properties. C Several physical properties o ...
Are there atoms in the air? Why or why not?
... Repeat After Me: Electron Definition: The negative part of the atom. It is a subatomic particle. Other Forms: Electrons ...
... Repeat After Me: Electron Definition: The negative part of the atom. It is a subatomic particle. Other Forms: Electrons ...
Periodic Table of Elements
... • Oxygen is the most abundant element in the earth’s crust and the 2nd most in the atmosphere. • Examples: S, Te, and Po ...
... • Oxygen is the most abundant element in the earth’s crust and the 2nd most in the atmosphere. • Examples: S, Te, and Po ...
File u1 sec2.2 slide show
... Q: What period is Nickel located? _____ Q: How many elements are in period 1? _____ ...
... Q: What period is Nickel located? _____ Q: How many elements are in period 1? _____ ...
Chem 115 POGIL Worksheet
... This ordering, however, seemed to place some elements out of sequence. A better arrangement, based on atomic number, became possible in 1913, when Henry G. J. Moseley found that the atomic numbers of elements could be determined experimentally from their characteristic x-ray frequencies. Today the ...
... This ordering, however, seemed to place some elements out of sequence. A better arrangement, based on atomic number, became possible in 1913, when Henry G. J. Moseley found that the atomic numbers of elements could be determined experimentally from their characteristic x-ray frequencies. Today the ...
elements and compounds - Hicksville Public Schools
... 9. What is the atomic number of Magnesium? ____________ 10. What is the atomic number of chlorine? _____________________ 11. What is the atomic number of sodium? _____________________ 12. What is the atomic mass of sodium? ________________________ 13. What is the atomic mass of aluminum? ___________ ...
... 9. What is the atomic number of Magnesium? ____________ 10. What is the atomic number of chlorine? _____________________ 11. What is the atomic number of sodium? _____________________ 12. What is the atomic mass of sodium? ________________________ 13. What is the atomic mass of aluminum? ___________ ...
Slide 1
... How did chemists begin to organize the known elements? How did Mendeleev organize his periodic table? How is the modern periodic table organized? What are three broad classes of elements? ...
... How did chemists begin to organize the known elements? How did Mendeleev organize his periodic table? How is the modern periodic table organized? What are three broad classes of elements? ...
Periodic Properties
... Atomic Size - the size of the atom decreases as you move from the left side of the chart to the right side of the chart; the size of the atom increases as you move down a column in the chart a. adding additional orbitals causes the size of the atom to increase as you move down the chart b. adding ad ...
... Atomic Size - the size of the atom decreases as you move from the left side of the chart to the right side of the chart; the size of the atom increases as you move down a column in the chart a. adding additional orbitals causes the size of the atom to increase as you move down the chart b. adding ad ...
Chapter 3: The Elements Eli and Ethan Objective: To learn about the
... ■ Ex: Water will always contain 8g of oxygen for every 1 g of hydrogen. This principle is known as the law of constant composition, meaning that a given compound always has the same composition, regardless of where it comes from. Based off of these observations, John Dalton, an English scientist off ...
... ■ Ex: Water will always contain 8g of oxygen for every 1 g of hydrogen. This principle is known as the law of constant composition, meaning that a given compound always has the same composition, regardless of where it comes from. Based off of these observations, John Dalton, an English scientist off ...
Topic 5: The periodic Table
... • How many electrons and protons does manganese (Mn) have? • How many neutrons does Manganese have? • How many electrons and protons does gold (Au) have? • How many neutrons does gold (Au) have? • How many electrons and protons does zirconium (Zr) have? • How many neutrons does zirconium (Zr) have? ...
... • How many electrons and protons does manganese (Mn) have? • How many neutrons does Manganese have? • How many electrons and protons does gold (Au) have? • How many neutrons does gold (Au) have? • How many electrons and protons does zirconium (Zr) have? • How many neutrons does zirconium (Zr) have? ...
Ch. 6 - The Periodic Table
... ◦ What are the trends among the elements for first ionization energy, ionic size, and electronegativity? The energy required to remove an electron from an atom is called ionization energy. The energy required to remove the first electron from an atom is called the first ionization energy. The ...
... ◦ What are the trends among the elements for first ionization energy, ionic size, and electronegativity? The energy required to remove an electron from an atom is called ionization energy. The energy required to remove the first electron from an atom is called the first ionization energy. The ...
Periodic Table and Trends
... The top, right-area of the periodic table has the smallest atomic radius (helium) Which would you assume to have the largest atomic radius: Al, Al+, or AlWhich would you assume to have the smallest atomic radius: C2+, C+, C, C-, C2- ...
... The top, right-area of the periodic table has the smallest atomic radius (helium) Which would you assume to have the largest atomic radius: Al, Al+, or AlWhich would you assume to have the smallest atomic radius: C2+, C+, C, C-, C2- ...
Lesson 1 - Scientist in Residence
... This lab introduces the periodic table, the structure of the atom, and how the positions of the elements in the periodic table relate to conduction and insulation. An element is a piece of matter in its simplest form. All matter (solid, liquid, gas) is made of atoms. Atoms join together to make mole ...
... This lab introduces the periodic table, the structure of the atom, and how the positions of the elements in the periodic table relate to conduction and insulation. An element is a piece of matter in its simplest form. All matter (solid, liquid, gas) is made of atoms. Atoms join together to make mole ...
Periodic Table of Elements
... "water-silver." Many periodic tables include the full name of element as well and color-code the elements based on their phase at room temperature (solid, liquid, or gas). ...
... "water-silver." Many periodic tables include the full name of element as well and color-code the elements based on their phase at room temperature (solid, liquid, or gas). ...
Year 11 Chemistry: Chapter 3 ~ The Periodic Table
... A naturally occurring sample of an element contains the same isotopes in the same proportions, regardless of its source. An average weight of the atom can be calculated using the relative isotopic masses with their abundances known as ______ _____________ and is given the symbol _______ . *The relat ...
... A naturally occurring sample of an element contains the same isotopes in the same proportions, regardless of its source. An average weight of the atom can be calculated using the relative isotopic masses with their abundances known as ______ _____________ and is given the symbol _______ . *The relat ...
Periodic trends
... Still highly reactive but not as much so as alkali metals (2 valence e-) ...
... Still highly reactive but not as much so as alkali metals (2 valence e-) ...
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.