Chemical Periodicity - Fort Thomas Independent Schools
... The metallic elements at the far left of the periodic table have low electronegativities. By contrast, the nonmetallic elements at the far right (excluding the noble gases), have high electronegativities. The electronegativity of cesium, a metal, the least electronegative element, is 0.7; the elect ...
... The metallic elements at the far left of the periodic table have low electronegativities. By contrast, the nonmetallic elements at the far right (excluding the noble gases), have high electronegativities. The electronegativity of cesium, a metal, the least electronegative element, is 0.7; the elect ...
Chapter 5
... Atom – the smallest particle of an element that retains its identity in a chemical reaction - Democritus, Greek philosopher, believed that atoms were indivisible and indestructible o No experimental support - Robert Dalton’s theory, using experimental methods, proposed: o All elements are composed o ...
... Atom – the smallest particle of an element that retains its identity in a chemical reaction - Democritus, Greek philosopher, believed that atoms were indivisible and indestructible o No experimental support - Robert Dalton’s theory, using experimental methods, proposed: o All elements are composed o ...
Q1: Isotopes of an element contain: A. the same atomic number and
... d Which has one more electron than a magnesium atom? A e Which is a group 2 element? B f How many different elements are shown? 7 Q6: Insert either INCREASE or DECREASE in the gaps to complete the sentences a. As you move down a group the ionization energy will decrease, as you move from right to le ...
... d Which has one more electron than a magnesium atom? A e Which is a group 2 element? B f How many different elements are shown? 7 Q6: Insert either INCREASE or DECREASE in the gaps to complete the sentences a. As you move down a group the ionization energy will decrease, as you move from right to le ...
The atom
... particles called atoms 2. Atoms can be neither created nor destroyed in chemical reactions 3. All atoms of a given element are identical 4. Atoms chemically combine in definite whole-number ratios to form compounds 5. Atoms of different elements have different masses ...
... particles called atoms 2. Atoms can be neither created nor destroyed in chemical reactions 3. All atoms of a given element are identical 4. Atoms chemically combine in definite whole-number ratios to form compounds 5. Atoms of different elements have different masses ...
Isotopes
... • Atoms of the same element with different atomic masses are called isotopes. • Atoms of the same element have the same properties. • But what causes the chemical properties of an atom? • So atoms of different isotopes of an element must have the same number of protons and electrons. • Whatever cau ...
... • Atoms of the same element with different atomic masses are called isotopes. • Atoms of the same element have the same properties. • But what causes the chemical properties of an atom? • So atoms of different isotopes of an element must have the same number of protons and electrons. • Whatever cau ...
Section 5.1 Review
... 2. _____ 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. (c) atomic number. (b) reactivity. (d) atomic mass. 3. _____ The modern periodic law states that (a) no two el ...
... 2. _____ 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. (c) atomic number. (b) reactivity. (d) atomic mass. 3. _____ The modern periodic law states that (a) no two el ...
Models of the Atom Intro
... Electrons have special rules…. • You can’t just shove all of the electrons into the first orbit of an electron. • Electrons live in something called shells or energy levels. ...
... Electrons have special rules…. • You can’t just shove all of the electrons into the first orbit of an electron. • Electrons live in something called shells or energy levels. ...
Unit 1: Atomic Structure & Electron Configuration
... A. Absorption Spectrum –when an e- absorbs energy, it moves from the ground state (most stable arrangement of e-) to an excited state (which is not stable) B. Emission Spectrum - when an e- emits energy, it falls from the excited state back to ground state, releasing energy in the form of electromag ...
... A. Absorption Spectrum –when an e- absorbs energy, it moves from the ground state (most stable arrangement of e-) to an excited state (which is not stable) B. Emission Spectrum - when an e- emits energy, it falls from the excited state back to ground state, releasing energy in the form of electromag ...
Atomic Structure
... • The electrons are arranged in energy levels within the electron cloud. • Each energy level or shell is labeled with a number or letter. For example K-Shell or energy level 1 • Each energy level or shell can hold a maximum number of electrons: #e- = 2n2 where n = energy level. Level 1 holds 2 elect ...
... • The electrons are arranged in energy levels within the electron cloud. • Each energy level or shell is labeled with a number or letter. For example K-Shell or energy level 1 • Each energy level or shell can hold a maximum number of electrons: #e- = 2n2 where n = energy level. Level 1 holds 2 elect ...
Basic atomic structure
... + Charge Used to identify an atom Equal to atomic number Included in mass number Same mass as a neutron Change in protons [RARE!] = change in element name and atomic mass ...
... + Charge Used to identify an atom Equal to atomic number Included in mass number Same mass as a neutron Change in protons [RARE!] = change in element name and atomic mass ...
Chapter 1
... B. Now for Some Neutrons C. Building Bigger Atoms D. Protons and Atomic Number *Notes-The number of protons in the nucleus of an atom give the element its _____________________. (also the number of electrons) ...
... B. Now for Some Neutrons C. Building Bigger Atoms D. Protons and Atomic Number *Notes-The number of protons in the nucleus of an atom give the element its _____________________. (also the number of electrons) ...
Goal 5 – Structure and Properties of Matter
... that occupies each level. It was impossible to predict the exact location of an electron within an atom, but that it was more likely to occur within a probable area called an electron cloud. Atomic Structure – the three parts of an atom are the protons (+), neutrons and the electrons. Protons and ne ...
... that occupies each level. It was impossible to predict the exact location of an electron within an atom, but that it was more likely to occur within a probable area called an electron cloud. Atomic Structure – the three parts of an atom are the protons (+), neutrons and the electrons. Protons and ne ...
Periodicity
... elements with the most similar properties were side by side. He left empty spaces for elements that had not yet been discovered. Later those elements were found to fit right in the spaces of Mendeleev’s table. In 1913, Henry Moseley (1887-1915), a British physicist, determined the nuclear charge (at ...
... elements with the most similar properties were side by side. He left empty spaces for elements that had not yet been discovered. Later those elements were found to fit right in the spaces of Mendeleev’s table. In 1913, Henry Moseley (1887-1915), a British physicist, determined the nuclear charge (at ...
Properties of Atoms and the Periodic Table
... 9. Atoms of the same element that have different numbers of neutrons are called (isotopes/electron clouds), 10. In the periodic table, elements are arranged by increasing atomic (power/number). 11. An electron dot diagram uses the symbol of an element and dots to represent the (quarks/electrons) in ...
... 9. Atoms of the same element that have different numbers of neutrons are called (isotopes/electron clouds), 10. In the periodic table, elements are arranged by increasing atomic (power/number). 11. An electron dot diagram uses the symbol of an element and dots to represent the (quarks/electrons) in ...
Physical properties
... Periodic Table Vocabulary Identify each word with its definition. Each word can only be used once. ...
... Periodic Table Vocabulary Identify each word with its definition. Each word can only be used once. ...
Ch_6_Notes_Periodic_Table
... the periodic table. As you move down a group in the periodic table, atomic ______ generally ________________. The atomic radius ______________________ from left to right across a period in the periodic table. Lithium has the _______________ atomic radius in the second period. As the number of electr ...
... the periodic table. As you move down a group in the periodic table, atomic ______ generally ________________. The atomic radius ______________________ from left to right across a period in the periodic table. Lithium has the _______________ atomic radius in the second period. As the number of electr ...
Topic 3 Review
... Electron shells and valence electrons a) Electron shells determine how an atom behaves when it encounters other atoms. b) The 1st shell can hold up to two electrons, and each shell thereafter can hold up to 8 electrons. Valence electrons are the electrons in the highest occupied energy level of an ...
... Electron shells and valence electrons a) Electron shells determine how an atom behaves when it encounters other atoms. b) The 1st shell can hold up to two electrons, and each shell thereafter can hold up to 8 electrons. Valence electrons are the electrons in the highest occupied energy level of an ...
Democritus John Dalton Joseph John (J.J.) Thomson Dimitri
... Model”) that placed electrons in specific energy levels (orbits) around the nucleus. When energized, electrons can jump from one orbit to another, then fall back to their stable (a.k.a. ...
... Model”) that placed electrons in specific energy levels (orbits) around the nucleus. When energized, electrons can jump from one orbit to another, then fall back to their stable (a.k.a. ...
Note Sheet 6 – Atomic Structure
... o Ex. 1 oxygen atom has _____ protons + neutrons o To figure out the number of neutrons subtract the _______________ from the _______________ o 16 – 8 = 8, so an oxygen atom has _____ neutrons ...
... o Ex. 1 oxygen atom has _____ protons + neutrons o To figure out the number of neutrons subtract the _______________ from the _______________ o 16 – 8 = 8, so an oxygen atom has _____ neutrons ...
Chemistry Test Review - Greenslime Home Page
... a. Change in temperature, bubbles produced, gas released, change in state of matter, color change, etc. 6. How many protons are in one molecule of NH4? Two molecules? a. 11 protons in one molecule b. 22 protons in 2 molecules 7. Describe the chemical formula: 4NaHCO3 a. 4 molecules of a compound con ...
... a. Change in temperature, bubbles produced, gas released, change in state of matter, color change, etc. 6. How many protons are in one molecule of NH4? Two molecules? a. 11 protons in one molecule b. 22 protons in 2 molecules 7. Describe the chemical formula: 4NaHCO3 a. 4 molecules of a compound con ...
The Atomic Model
... NOT arranged in neat orbits, but can be discussed only by the probability of where they are. (Electron Cloud) ...
... NOT arranged in neat orbits, but can be discussed only by the probability of where they are. (Electron Cloud) ...
ppt - Faculty
... number of protons), the neutron number, N, and the mass number, A, where A = Z + N. • The convention for designating nuclei is by atomic number, Z, and mass number, A, as well as its chemical symbol. The neutron number is given by N = A - Z. ...
... number of protons), the neutron number, N, and the mass number, A, where A = Z + N. • The convention for designating nuclei is by atomic number, Z, and mass number, A, as well as its chemical symbol. The neutron number is given by N = A - Z. ...