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trends in the periodic table worksheet use your knowledge of the period…

Question

trends in the periodic table worksheet
use your knowledge of the periodic table trends to answer the following question.
1 why does fluorine has high ionization energy than iodine?
2 why do elements in the same group have the same properties?
3 what characteristics do metalloids have?
4 why do atoms get smaller as you move from left to right in the periodic table?
5 which is the smallest atom in group 15 (va or 5a)?
6 which is the smallest atom in period 4?
7 which is the smallest atom in group 11 (ib or 1b)?
8 which is the largest atom in period 2?
9 indicate whether the following properties increase or decrease from left to right of the periodic table.
a atomic radius (exclude noble gases):
b first ionization energy:
c electronegativity:
10 provide the element name and chemical symbol.
a period 5, group 6 (vib or 6b):
b period 6, group 1 (ia or 1a):
c period 4, group 7 (vii b or 7b):
d period 4, group 14 (iv a or 4a):
e period 2, group 10 (iia or 2a):
f period 5, group 18 (viiia or 8a):
chemistrylearner.com

Explanation:

Brief Explanations

The problem is about the periodic table and its trends, which falls under Chemistry, a subfield of Natural Science. For example, question 1: Fluorine has a smaller atomic radius than iodine (same group, F is above I). Smaller radius means electrons are closer to the nucleus, so more energy is needed to remove an electron (ionization energy). Question 2: Elements in the same group have the same number of valence electrons, which determines chemical properties. Question 3: Metalloids have properties between metals and non - metals, e.g., semiconductivity, some metallic and non - metallic physical/chemical traits. Question 4: As you move left - to - right in a period, the number of protons increases (nuclear charge), pulling electrons closer, so atomic size decreases. Question 5: In Group 15, the topmost element (nitrogen) has the smallest radius (atomic size decreases top - to - bottom in a group? No, wait, atomic size increases top - to - bottom. Wait, no: in a group, as you go down, atomic size increases. So the smallest in Group 15 is nitrogen (N), as it's the topmost. Question 6: In Period 4, atomic size decreases left - to - right, so the rightmost non - noble gas? Wait, Period 4 elements: from K to Kr. The smallest is Kr? No, noble gases have larger radii? Wait, no, when considering atomic radius (excluding noble gases for some trends), but for atomic size, in a period, left - to - right, effective nuclear charge increases, so size decreases. So in Period 4, the smallest atom is krypton? Wait, no, the elements in Period 4: K, Ca, Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, Ga, Ge, As, Se, Br, Kr. The atomic radius decreases from K to Br, then Kr has a larger radius (noble gas). So the smallest in Period 4 (excluding noble gases? No, the question doesn't exclude. Wait, the question is "Which is the smallest atom in Period 4?". So among all, the rightmost with the highest nuclear charge. Br? Wait, no, Kr is a noble gas, but its atomic radius is measured differently (van der Waals radius). But in terms of atomic radius (covalent radius), Br has a smaller radius than Kr. Wait, maybe the question considers the general trend: in a period, atomic size decreases left - to - right, so the last element (Kr) but maybe the question expects the non - noble gas? Wait, no, let's check. Question 7: Group 11: Cu, Ag, Au. Atomic size increases down the group, so the smallest is Cu (copper). Question 8: Period 2: Li, Be, B, C, N, O, F, Ne. Atomic size decreases left - to - right, so the largest is Li (lithium). Question 9a: Atomic radius (exclude noble gases) decreases left - to - right. 9b: First ionization energy increases left - to - right (with exceptions, but overall trend). 9c: Electronegativity increases left - to - right. Question 10a: Period 5, Group 6: the element is molybdenum (Mo). 10b: Period 6, Group 1: cesium (Cs). 10c: Period 4, Group 7: manganese? Wait, no, Group 7 in Period 4: Mn? Wait, Group 7 (VII B) in Period 4 is Mn? No, Group 7 (VII B) elements: Mn (Period 4), Tc (Period 5), Re (Period 6), Bh (Period 7). So Period 4, Group 7 is manganese (Mn)? Wait, no, Group 7 (VII B) has elements with valence electrons? Wait, Group 7 (old numbering: VII B) is now Group 7. So Period 4, Group 7: Mn (manganese). 10d: Period 4, Group 14: Ge (germanium). 10e: Period 2, Group 10: Wait, Group 10 in Period 2: there is no Group 10 in Period 2. Wait, Period 2 elements: Li, Be, B, C, N, O, F, Ne. Group 10 is Ni, Pd, Pt, etc. So Period 2, Group 10: no element. Wait, maybe a typo? Maybe Group 2? If it's Group 2, Period 2: Be. But the question says Group 10 (…

Answer:

  1. Fluorine has a smaller atomic radius than iodine (same group, F is above I). Smaller radius means electrons are closer to the nucleus, so more energy is needed to remove an electron (ionization energy).
  2. Elements in the same group have the same number of valence electrons, which determines chemical properties.
  3. Metalloids have properties between metals and non - metals, e.g., semiconductivity, some metallic and non - metallic physical/chemical traits.
  4. As you move left - to - right in a period, the number of protons increases (nuclear charge), pulling electrons closer, so atomic size decreases.
  5. Nitrogen (N)
  6. Krypton (Kr) (Note: May need to re - evaluate based on radius type, but following left - to - right trend)
  7. Copper (Cu)
  8. Lithium (Li)
  9. a) Decrease; b) Increase; c) Increase
  10. a) Molybdenum (Mo); b) Cesium (Cs); c) Manganese (Mn); d) Germanium (Ge); e) (No element in Period 2, Group 10; possible typo, if Group 2: Beryllium (Be)); f) Xenon (Xe)

(Note: Some answers may need further verification with precise atomic radius data and periodic table trends, especially for noble gases and specific element positions.)