Review Periodic Table Section

In the modern Periodic Table, the elements are arranged according to oxidation number atomic number mass number atomic mass The element found in Group 13 and Period 2 is   Mg Al B Be Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms' atomic numbers number of principal energy levels number of valence electrons atomic masses Which compound contains an alkali metal and a halogen?   Rb₂S CaCl₂ CaS RbCl In the ground state, atoms of the elements in Group 15 of the Periodic Table all have the same number of neutrons in the nucleus electrons in the valence shell occupied principal energy levels filled principal energy levels   Which two elements have the most similar chemical properties? K and Cl K and S K and Ca K and Na As the atoms of the metals of Group 1 in the ground state are considered in order from top to bottom, the number of occupied principal energy levels   increases decreases remains the same   Which represents the correct electron configuration of a Group 14 element in the ground state? 2-3 2-7-5 2-8-4 2-8-8-1 At which location in the Periodic Table would the most active metallic element be found? in Group 1 at the bottom in Group 17 at the top in Group 17 at the bottom in Group 1 at the top   10) Atoms of metallic elements tend to lose electrons and form negative ions gain electrons and form negative ions gain electrons and form positive ions lose electrons and form positive ions   Atoms that are noble gases metals nonmetals metalloids Which element is considered malleable? sulfur radon gold hydrogen As elements in Group 15 of the Periodic Table are considered in order from top to bottom, the metallic character of each successive element generally   remains the same decreases increases Which element in Group 15 would most likely have luster and good electrical conductivity? As N P Bi What group in the Periodic Table contains the most active metals? 7 17 1 11 Which properties are characteristic of nonmetals? low thermal conductivity and low electrical conductivity high thermal conductivity and high electrical conductivity low thermal conductivity and high electrical conductivity   high thermal conductivity and low electrical conductivity Which Period 3 element has the least metallic character? Most NM   Na Mg Al Si Which element with a high first ionization energy would most likely be a metal with a high electronegativity metal with a low electronegativity nonmetal with a high electronegativity nonmetal with a low electronegativity diatomic 7: All Nonmetals H₂ O₂ F₂ Cl₂ Br₂ I₂ N₂ 19) Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having   fewer principal energy levels a smaller nuclear charge more principal energy levels a larger nuclear charge Which atom has the largest atomic radius?   Na 190 K 235 Mg 160 Ca 197 As the elements in Group 2 are considered in order of increasing atomic number, the atomic radius of each successive element increases. This increase is primarily due to an increase in the number of   occupied principal energy levels electrons in the outermost shell unpaired electrons neutrons in the nucleus   As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the atomic radius of each successive element compare?   The relative electronegativity increases and the atomic radius increases. The relative electronegativity decreases and the atomic radius increases. The relative electronegativity decreases and the atomic radius decreases. The relative electronegativity increases and the atomic radius decreases. As a sulfur atom gains electrons, its radius remains the same   decreases increases The highest ionization energies in any period are found in Group 1 2 17 18 Which element in Period 2 has the greatest tendency to gain electrons? F Ne C Li As the elements in Group 18 are considered in order of increasing atomic number, the ionization energy of each successive element decreases increases remains the same   Which properties are characteristic of the Group 1 metals? low reactivity and the formation of unstable compounds high reactivity and the formation of stable compounds high reactivity and the formation of unstable compounds low reactivity and the formation of stable compounds   Which of the following is the atomic number of an alkali metal? 13 10 11 12 Which group contains elements with a total of two electrons in the outermost principal energy level? 2 18 16 14 Which element is a member of the halogen family? K B Cl S Which element exhibits a crystalline structure at STP? iodine fluorine bromine chlorine Which halogens are gases at STP? chlorine and fluorine chlorine and bromine iodine and fluorine iodine and bromine   What is the total number of electrons found in the valence shell of a halogen in the ground state? 1 2 3. 7   8 Which electron-dot symbol could represent a noble gas? X X X X Which element exists as monatomic molecules at STP? hydrogen nitrogen chlorine argon