Unit Bohr Model and Electromagnetic Radiation - Jones
... 1. Gaining energy results in the electron moving from its ground state to a higher energy level. 2. When the electron moves to a lower energy level, it releases the energy difference in the two levels as electromagnetic radiation (emissions spectrum). Chm.1.3 Understand the physical and chemical pro ...
... 1. Gaining energy results in the electron moving from its ground state to a higher energy level. 2. When the electron moves to a lower energy level, it releases the energy difference in the two levels as electromagnetic radiation (emissions spectrum). Chm.1.3 Understand the physical and chemical pro ...
Name
... 1. Which of these elements is a MORE reactive nonmetal? 2. Which of these elements has a LOWER ionization energy? 3. Which of these elements has a LOWER electron affinity? 4. Which of these atoms is a BIGGER? 5. Which of these elements has a HIGH ionization energy? 6. Which of these elements is a MO ...
... 1. Which of these elements is a MORE reactive nonmetal? 2. Which of these elements has a LOWER ionization energy? 3. Which of these elements has a LOWER electron affinity? 4. Which of these atoms is a BIGGER? 5. Which of these elements has a HIGH ionization energy? 6. Which of these elements is a MO ...
Metals
... Ch9.5 Naming Acids and Bases (Discuss these in more detail later) Acids: A compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water. (The names of compounds can change when acids are present). The name of an acidic compound depends on the type of a ...
... Ch9.5 Naming Acids and Bases (Discuss these in more detail later) Acids: A compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water. (The names of compounds can change when acids are present). The name of an acidic compound depends on the type of a ...
Periodic Trends
... For the first ionization energy, going across the periodic table the ionization energy will generally increase. This is because the nuclear charge increases, pulling the valance electrons tighter to the nucleus. Going down the periodic table the ionization decreases because the electrons are further ...
... For the first ionization energy, going across the periodic table the ionization energy will generally increase. This is because the nuclear charge increases, pulling the valance electrons tighter to the nucleus. Going down the periodic table the ionization decreases because the electrons are further ...
U1 Periodic Trends - Alliance Ouchi-O`Donovan 6
... classification of the elements and the periodic law using a deck of special element cards. The real properties of the elements, but not their names or symbols, are written on these cards. As the cards are arranged and rearranged based on logical trends in some of these properties, the nature of the ...
... classification of the elements and the periodic law using a deck of special element cards. The real properties of the elements, but not their names or symbols, are written on these cards. As the cards are arranged and rearranged based on logical trends in some of these properties, the nature of the ...
The Periodic Table
... in increasing atomic number so elements with similar properties fall in the same group. Note: Ar and K both in according to atomic number, not atomic mass ...
... in increasing atomic number so elements with similar properties fall in the same group. Note: Ar and K both in according to atomic number, not atomic mass ...
Review sheet Atomic Structure, Electron Configuration, and Periodic
... Know that main group elements in the same group have similar properties, the same number of valence electrons and the same oxidation number. Understand that reactivity increases as you go down within a group for metals and decreases for nonmetals. Identify periods as horizontal rows on the periodic ...
... Know that main group elements in the same group have similar properties, the same number of valence electrons and the same oxidation number. Understand that reactivity increases as you go down within a group for metals and decreases for nonmetals. Identify periods as horizontal rows on the periodic ...
Chapter 6 Review
... ________ 12. Removing one electron from an atom results in the formation of a positive ion with a 1! charge. ________ 13. An anion has more electrons than protons. ________ 14. Elements with a high electronegativity value tend to form positive ions. ...
... ________ 12. Removing one electron from an atom results in the formation of a positive ion with a 1! charge. ________ 13. An anion has more electrons than protons. ________ 14. Elements with a high electronegativity value tend to form positive ions. ...
VIBRATIONS AND WAVES
... The s orbital holds a maximum of two electrons. groups 13-18 Group 18 elements have both their s orbitals and p orbitals completely filled with electrons. This configuration is very stable, thus, the group 18 elements are very unreactive. ...
... The s orbital holds a maximum of two electrons. groups 13-18 Group 18 elements have both their s orbitals and p orbitals completely filled with electrons. This configuration is very stable, thus, the group 18 elements are very unreactive. ...
Periodic Table
... Reactivity varies; but some are so unreactive that they exist free in nature (ex/ Platinum & Gold) ...
... Reactivity varies; but some are so unreactive that they exist free in nature (ex/ Platinum & Gold) ...
Periodic Table
... to share when they are bonded • Nonmetals, metalloids and metals • Nitrogen makes up over ¾ of the atmosphere. • Nitrogen and phosphorus are both important in living things. • Most of the world’s nitrogen is not available to living things. • The red stuff on the tip of matches is phosphorus. ...
... to share when they are bonded • Nonmetals, metalloids and metals • Nitrogen makes up over ¾ of the atmosphere. • Nitrogen and phosphorus are both important in living things. • Most of the world’s nitrogen is not available to living things. • The red stuff on the tip of matches is phosphorus. ...
Periodic Table Name: Practice Review H
... grouped in A) periods C) horizontal rows E) horizontal families ...
... grouped in A) periods C) horizontal rows E) horizontal families ...
periodicity
... • Anion – a negatively charged ion (i.e. F1-) • Ionic radius increases from right to left across a period and increases from top to bottom ...
... • Anion – a negatively charged ion (i.e. F1-) • Ionic radius increases from right to left across a period and increases from top to bottom ...
Evidence Statements: HS-PS1-1
... HS-PS1-1 Students who demonstrate understanding can: HS-PS1-1. ...
... HS-PS1-1 Students who demonstrate understanding can: HS-PS1-1. ...
Ch. 4.3 – Distinguishing Among Atoms
... A periodic table is an arrangement of elements in which the elements are separated into groups based on a set of repeating properties. A periodic table allows you to easily compare the properties of one element (or a group of elements) to another element (or group of elements). ...
... A periodic table is an arrangement of elements in which the elements are separated into groups based on a set of repeating properties. A periodic table allows you to easily compare the properties of one element (or a group of elements) to another element (or group of elements). ...
Ch.6 Periodic Trends - MrsSavallisChemistry
... 3. Name the three broad classes of elements. 4. Identify each property below as more characteristic of a mental or a nonmetal. a. a gas b. brittle c. malleable d. poor conductor of electric current e. shinny 5. In general, how are metalloids different from metals and nonmetals? 6. Elements in the sa ...
... 3. Name the three broad classes of elements. 4. Identify each property below as more characteristic of a mental or a nonmetal. a. a gas b. brittle c. malleable d. poor conductor of electric current e. shinny 5. In general, how are metalloids different from metals and nonmetals? 6. Elements in the sa ...
Chapter 3: The Elements Eli and Ethan Objective: To learn about the
... 2) Elements are made up tiny particles called atoms. All atoms of a given elements are identical.The atoms of a given element are different from those of any element. Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative number ...
... 2) Elements are made up tiny particles called atoms. All atoms of a given elements are identical.The atoms of a given element are different from those of any element. Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative number ...
The Periodic Table
... 16. Describe periodic trends for first ionization energy and electronegativity 17. Ionization Energy: define, label trend down a group and across a period, in which corner would largest/smallest I.E. be found, list the reason(s) why the trend exists (shielding effect is a huge factor!) 18. Explain w ...
... 16. Describe periodic trends for first ionization energy and electronegativity 17. Ionization Energy: define, label trend down a group and across a period, in which corner would largest/smallest I.E. be found, list the reason(s) why the trend exists (shielding effect is a huge factor!) 18. Explain w ...
graphing atomic properties
... 6. Circle the atom that would require the LEAST amount of energy to remove an ea. magnesium, chlorine, silicon b. lithium, cesium, potassium c. fluorine, iodine, chlorine d. calcium, bromine, cobalt 7. Circle the atom that would require the MOST amount of energy to remove an ea. lithium, potassium, ...
... 6. Circle the atom that would require the LEAST amount of energy to remove an ea. magnesium, chlorine, silicon b. lithium, cesium, potassium c. fluorine, iodine, chlorine d. calcium, bromine, cobalt 7. Circle the atom that would require the MOST amount of energy to remove an ea. lithium, potassium, ...
Atom and periodic table review
... High ionization energy, do not want to form cations. High electron affinity, want to form anions when bonded to metals. Mostly gases, except for bromine (liquid), and carbon, phosphorus, selenium, and iodine which are solids. Metalloids— zig zag line between the metals and nonmetals on periodic tabl ...
... High ionization energy, do not want to form cations. High electron affinity, want to form anions when bonded to metals. Mostly gases, except for bromine (liquid), and carbon, phosphorus, selenium, and iodine which are solids. Metalloids— zig zag line between the metals and nonmetals on periodic tabl ...
ionic compound - East Penn School District
... Published almost the same element classification scheme as Mendeleev but did not receive credit because Mendeleev revealed his first and Mendeleev was more successful at demonstrating its usefulness ...
... Published almost the same element classification scheme as Mendeleev but did not receive credit because Mendeleev revealed his first and Mendeleev was more successful at demonstrating its usefulness ...
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.