1. II. Periodic Table

2. The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order of increasing atomic number.
Mendeleev’s original table was according to mass. This was changed when Moseley discovered atomic number.
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3. Atomic mass is found on the Periodic Table of the Elements
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4. Regents Question: 01/03 #3
In which list are the elements arranged in order of increasing atomic mass?
Cl, K, Ar
Fe, Co, Ni
Te, I Xe
Ne, F, Na þ
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5. Elements can be classified by their properties and located on the Periodic Table as metals, nonmetals, metalloids or semimetals (B, Si, Ge, As, Sb, Te), and noble gases.
Nonmetals on the right
Metals on the left
Metalloids or semimetals
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6. Comparing the physical properties of metals and nonmetals
Make up 2/3 of the periodic table
Low ionization energy: amount of energy needed to remove valence electron Low electronegativity: desire for more electrons.
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7. Solid at room temperature except. mercury (Hg)
*Solid at room temperature except mercury (Hg) *Good conductors of heat and electricity *Malleable – can be hammered into shapes (thin sheets) *Ductile – can be pulled into wires *Lose electrons to form (+) ions *Most metallic element is in the lower left corner of the periodic table. Francium (Fr)
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8. Comparing the physical properties of metals and nonmetals
Many different states (phases)
Gases: Hydrogen (H), Oxygen (O), Nitrogen (N), Fluorine (F), Chlorine (Cl), All of group 18 (noble gases)
Helium (He), Neon (Ne) Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn)
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9. Bromine (Br) - the only liquid nonmetal at room temperature
*Bromine (Br) - the only liquid nonmetal at room temperature *Poor conductors of heat and electricity and brittle – breaks when hit *High ionization and electronegativity. *Gain electrons to form(-) ions
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10. Metalloids: having both metallic and non metallic properties B(boron), Si(silicon), Ge(germanium), As(arsenic), Sb(Antimony), Te(tellurium) and At(astatine)
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11. Regents Question: 01/03 # 37
Which list of elements contains two metalloids?
Si, Ge, Po, Pb
As, Bi, Br, Kr
Si, P, S, Cl
Po, Sb, I, Xe þ
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12. Regents Question: 06/03 # 6
Which is a property of most nonmetallic solids?
(1) high thermal conductivity
(2) high electrical conductivity
(3) brittleness
(4) malleability þ
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13. For Groups 1, 2, and on the Periodic Table, elements within the same group have the same number of valence electrons (helium is an exception) and therefore similar chemical properties.
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14. They are in the same group
Regents Question: 06/03 # 53-54
Given: Samples of Na, Ar, As, Rb
Which two of the given elements have the most similar chemical properties?
Explain your answer in terms of the Periodic Table of the Elements.
Na and Rb
They are in the same group
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15. Group numbers and family names Groups are elements that share similar characteristic
Group 1 Alkali Metals
Very reactive metals in water, always found as compounds in nature
Francium is the most reactive metal
1 valence electron - lose 1 electron to form +1 ions
Group 2 Alkaline Earth Metals
Reactive metals, always found as compounds in nature
2 valence electrons - lose 2 electron to form +2 ions
Group 3-12 Transition Metals
Forms colored solutions
Fills two valence shells at one time
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16. Groups continued Group 17 Halogens Groups 18 Noble Gases
Reactive nonmetals
7 valence electrons - gain 1 electron to form –1 ions
Groups 18 Noble Gases
Not reactive – do not form ions
Filled, stable valence shell (8 electrons except He which has 2)
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17. Regents Question: 01/03 #6
Which Group of the periodic Table contains atoms with a stable outer electron configuration? 1 8 16 18 þ
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18. STP is standard temperature and pressure
Regents Question: 02/06 #6
Which element is classified as a noble gas at STP?
Hydrogen
Oxygen
Neon
Nitrogen þ
STP is standard temperature and pressure
0ºC (273K) and 1 atm (101.3kPa)
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19. The succession of elements within the same group demonstrates characteristic trends: differences in atomic radius, first ionization energy, ionic radius, electronegativity, metallic/nonmetallic properties.
Going down a group, there are more shells separating the nucleus from the valence electrons
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20. The succession of elements across the same period demonstrates characteristic trends: differences in atomic radius, ionic radius, electronegativity, first ionization energy, metallic/nonmetallic properties.
Going across a period, there are more protons pulling on the valence electrons
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21. Reference Table S
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22. Trends in First Ionization Energy
First ionization energy is the amount of energy needed to remove the most loosely held electron from an atom in the gaseous state.
Going down a group, first ionization energy decreases because there are more shells and the electron being attracted is far from the protons
Going across a period, first ionization energy increases because there are more protons in the nucleus to attract the electrons. (same number of shells)
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23. Regents Question: 01/03 #7
From which of these atoms in the ground state can a valence electron be removed using the least amount of energy?
Nitrogen
Carbon
Oxygen
Chlorine þ
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24. Trends in Electronegativity
Electronegativity – the relative ability of an atom to attract electrons (in a chemical bond)
Fluorine (F) has the highest electronegativity and is assigned the value 4.0
Francium (Fr) has the lowest electronegativity.
Going down a group, electronegativity decreases because there are more shells and the electron being attracted is far from the protons
Going across a period, electronegativity increases because there are more protons in the nucleus to attract the electrons. (same number of shells)
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25. Regents Question: 01/03 #10
The strength of an atom’s attraction for the electrons in a chemical bond is the atom’s
Electronegativity
Ionization energy
Heat of reaction
Heat of formation þ
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26. Regents Question: 06/02 #11
Which of the following atoms has the greatest tendency to attract electrons?
Barium
Beryllium
Boron
Bromine þ
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27. Trends in Atomic Radius
Atomic Radius – half the distance between two nuclei or the distance between the nucleus and outer( valence) electrons
Going down a group, the atomic radius increases because there are more principal energy levels (shells)
Going across a period, the atomic radius decreases because there are more protons pulling the valence shell closer
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28. Atomic Radius
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29. Regents Question: 06/03 #38 Check Table S þ
Which list of elements is arranged in order of
increasing atomic radii?
Li, Be, B, C
(2) Sr, Ca, Mg, Be
(3) Sc, Ti, V, Cr
(4) F, Cl, Br, I
Check Table S þ
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30. Forming Ions – making atoms happy
Atoms gain or lose electrons to complete their outer shell
A noble gas configuration
A complete octet
8 electrons
Metals lose electrons to form positive (+) ions
Nonmetals gain electrons to form negative (-) ions
Ionic Radius
A negative ion is always larger than its original atom.
A positive ion is always smaller than its original atom.
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31. Regents Question: 06/03 #37
What is the total number of electrons in a Cu + ion?
(1) 28
(2) 29
(3) 30
(4) 36 þ
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32. Ionic Radius in Metals Sodium (Na) is a metal
Electron configuration 2-8-1
(11 protons and 11 electrons)
Loses 1 electron in its valence shell
A sodium atom becomes a sodium ion
Na+
2-8 (10 electrons but 11 protons)
Same electron configuration as a noble gas (Ne) but has more protons. Electrons are pulled in much closer so the radius decreases.
2+ ions are even smaller than + ions
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33. Ionic Radius in Nonmetals
Notice-name of negative ions end in IDE
Chlorine (Cl) is a nonmetal
Electron configuration 2-8-7
(17 protons and 17 electrons)
Gains 1 electron in its valence shell
A chlorine atom becomes a chloride ion
Cl-
(18 electrons but only 17 protons)
Same electron configuration as a noble gas (Ar) but has fewer protons. Electrons repel each other and the radius increases.
2- ions are even larger than – ions
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34. Regents Question: 06/03 #60
As a neutral sulfur atom gains two electrons, what happens to the radius of the atom?
It gets bigger
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35. Regents Question: 06/03 #61
After a neutral sulfur atom gains two electrons, what is the resulting charge of the ion? 2-
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36. Regents Question: 08/02 #23
Which electron configuration is correct for a
sodium ion?
(1) 2–7
(2) 2–8
(3) 2–8–1
(4) 2–8–2 þ
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37. Regents Question: 08/02 #47
Which ion has the same electron configuration as an atom of He?
(1) H–
(2) O2–
(3) Na+
(4) Ca2+
- means gains 1 electron
2- means gains 2 electrons
+ means loses 1 electron
2+ means loses 2 electrons þ
GIN LIP
Gaining electrons makes Ions Negative
Losing electrons makes Ions Positive
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38. Regents Question: 06/02 #39
Which of the following ions has the smallest radius? F-
Cl- K+
Ca2+ þ
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39. Regents Question: 06/02 #30
As an atom becomes an ion, its mass number
Decreases
Increases
Remains the sam þ
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40. Regents Question: 06/02 #10
Compared to the radius of a chlorine atom, the radius of a chloride ion is
Larger because chlorine loses an electron
Larger because chlorine gains an electron
Smaller because chlorine loses an electron
Smaller because chlorine gains an electron þ
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41. Trends in Metallic Properties
Metals lose electrons to complete their outer shells form positive (+) ions
Metals have low electronegativity and low first ionization energy
Metallic properties (characteristics) decrease as you go to the right across a period
Metallic properties increase as you go down a group
Going towards Francium (Fr), metallic properties increases.
Anything that increases an atom’s ability to lose electrons, increase the atoms metallic characteristics.
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42. Trends in Nonmetallic Properties
Nonmetals want to gain electrons and form negative (-) ions
Nonmetals have high electronegativity and high first ionization energy
Nonmetallic properties (characteristics) increase as you go to the right across a period
Nonmetallic properties decrease as you go down a group
Going towards Fluorine (F), nonmetallic properties increases.
Anything that increases an atom’s ability to gain electrons, increase the atoms nonmetallic characteristics.
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43. Regents Question: 06/02 #32
Which of the following Group 15 elements has the greatest metallic character?
Nitrogen
Phosphorous
Antimony
Bismuth þ
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44. Regents Question: 06/02 #5
Which are two properties of most nonmetals?
High ionization energy and poor electrical conductivity
High ionization energy and good electrical conductivity
Low ionization energy and poor electrical conductivity
Low ionization energy and good electrical conductivity þ
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45. Regents Question: 06/02 #67-69 Element Atomic Number Electronegativity
Beryllium 4
1.6
Boron 5 2
Carbon 6
2.6
Fluorine 9
4.0
Lithium 3
1.0
Oxygen 8
3.4
On the grid in your answer booklet, set up a scale for electronegativity on the y-axis. Plot the data by drawing the best-fit line.
Using the graph, predict the electronegativity of nitrogen
For these elements, state the trend in electronegativity in terms of atomic number.
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46. Regents Question: cont’d
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47. Regents Question: cont’d1 2 3 4
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48. Regents Question: Cont’d1 2 3 4
3.0
On the grid in your answer booklet, set up a scale for electronegativity on the y-axis. Plot the data by drawing the best-fit line.
Using the graph, predict the electronegativity of nitrogen
For these elements, state the trend in electronegativity in terms of atomic number.
As the atomic number increases, the electronegativity increases.
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49. Elements can be differentiated by their physical properties
Elements can be differentiated by their physical properties. Physical properties of substances, such as density, conductivity, malleability, solubility, and hardness, differ among elements.
Density=mass/volume
A physical property is one which does not change the identity of the substance when tested.
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50. Elements can be differentiated by chemical properties
Elements can be differentiated by chemical properties. Chemical properties describe how an element behaves during a chemical reaction.
When testing a chemical property, the substance may change into another substance.
The number of atoms an element combines with is an important chemical property:
NaCl CaCl2 AlCl3 CCl4
HCl H2O NH3 CH4
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51. Buckminsterfullerene
Some elements exist in two or more forms in the same phase. These forms differ in their molecular or crystal structure, and hence in their properties. These are called allotropes.
Allotropes of oxygen
Allotropes of carbon
Oxygen ( O2 )
Graphite
Ozone ( O3 )
Diamond
Buckminsterfullerene
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