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25 Cards in this Set
- Front
- Back
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Define the term Periodic Law
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When elements are arranged in order of increasing atomic number, elements with similar properties occur at regular intervals.
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Define the term 'Main group element'
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An element in the A groups (1A, 2A, 3A - 8A) of the Periodic Table.
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Define the term 'Inner transition element'
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Elements which appear at the bottom of the Periodic Table and belong between columns 3 & 4 of the transition elements.
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Define the term ' Transition element'
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Elements in the B columns of the Periodic Table.
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Define the term 'Group'
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A vertical column of elements in the Periodic Table.
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Define the term 'Period'
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A horizontal row of elements in the Periodic Table.
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Define the term 'Metal'
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An element that has the characteristic properties of lustre, thermal and electrical conductivity and malleability. All metals are solid at room temperature (except mercury).
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Define the term 'Non-metal'
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An element characterised by the absence of the properties of metals. Many of the non-metals are gases and solids.
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Describe the difference between a metal and a non-metal
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Metals have the properties of lustre, thermal and electrical conductivity and malleability and non-metals do not.
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Explain the organisation of electrons in electron orbitals
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(1) Orbitals fill in order of increasing energy - lowest to highest (2) Each orbital holds 2 electrons (3) Each is half-filled before any are completely filled
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Describe the concept of electron configuration.
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An electron configuration is a statement of how many electrons an atom has in each of its electron sub-shells.
Hydrogen = H1s(1) Beryllium = Be1s(2)2s(2) (Numbers in brackets are superscript) |
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Use the Periodic Table to predict the electron configuration of an element.
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Nitrogen, atomic no. 7, has 7 electrons in its neutral atoms. 2 electrons in the 1s orbital; 2 in the 2s; 1 each in the 2px, 2py, 2pz.
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Draw the Lewis dot structure depicting the electron configuration of an element
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The outermost electrons, valence electrons, are represented in Lewis dot diagrams.
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Write the Lewis dot structure for the element that has the following ground-state electron configuration. What is the name of this element?
1s2 2s2 2px2 2py2 2pz2 3s2 3px1. |
Aluminum (Al)
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True or False
Elements in the same column of the Periodic Table have the same outer-shell configuration? |
True
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True or False
All Group 1A elements have one electron in their valence shell? |
True
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True or False
All Group 6A elements have six electrons in their valence shell? |
True
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True or False
All Group 8A elements have eight electrons in their valence shell? |
False
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True or False
Period 1 of the Periodic Table has one element, period 2 has two elements, period 3 has three and so forth? |
False
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True or False
Period 2 results from filling the 2s and 2p orbitals and, therefore, there are eight elements in period 2. |
True
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True or False
Period 3 results from filling the 3s, 3p and 3d orbitals and, therefore, there are nine elements in period 3. |
False
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True or False
The main-group elements are s block and p block elements. |
True
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How many electrons are in the outer shell of the following elements?
(a) Si (b) Br (c) P (d) K (e) He |
(a) Silicon Group 4A. 4 valence.
(b) Bromine Group 7A. 7 valence. (c) Phosphorus Group 5A. 5 valence. (d) Potassium Group 1A. 1 valence. (e) Helium Group 8A. 2 valence. |
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How many electrons are in the outer shell of the following elements?
(f) Ca (g) Kr (h) Pb (i) Se (j) O |
(f) Calcium Group 2A. 2 valence.
(g) Krypton Group 8A. 8 valence. (h) Lead Group 4A. 4 valence. (i) Selenium Group 6A. 6 valence. (j) Oxygen Group 6A. 6 valence. |
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Write a summary of an electron configuration.
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1s (s=2)
2s 2p (p=6) 3s 3p 3d (d=10) 4s 4p 4d 4f (f=14) 5s 5p 5d 5f 6s 6p 6d 7s 7p 8s |
