Download
1 / 38
380 likes | 498 Views
Final Jeopardy. Final Jeopardy Semester 1 Knowledge. Final Jeopardy. Ionic X > 1.7 Polar Covalent 1.7 X .5 Pure Covalent X < .5 .
E N D
Final Jeopardy Final Jeopardy Semester 1 Knowledge
Final Jeopardy Ionic X > 1.7 Polar Covalent 1.7 X .5 Pure Covalent X < .5 Write down the 3 divisions and numbers that you must use after you subtract the Electronegativity numbers between 2 atoms in a molecule.
$200 Properties of the elements that repeat consistently across the periods, determined by electron configuration What is the definition of Periodic Properties?
$400 Amount of pull the valence electrons feel from protons in the nucleus What is the effective Nuclear Charge (Z)?
$600 Stays the same The effective nuclear charge trend for going down a family…
$800 Goes up, because protons increase while shielding electrons stays the same Going across a period, the effective nuclear charge...
$1000 Atomic size What is the size of an atom called?
$200 Effective nuclear charge and energy levels What are factors which affect the size of an atom and how they affect it ?
$400 Increases due to the adding of more energy levels Trend of atomic size going down a family…
$600 Trend of atomic size going across a period What Decreases due to energy level staying the same, while effective nuclear charge increases (more pull on valence electrons)?
$800 Ionization Energy What is the energy needed to move an electron?
$1000 The effective nuclear charge and atom size What are factors which affect ionization energy and how they affect it ?
$200 Trend of ionization energy going down a family What decreases (easier to remove) because size is bigger, so valence electrons are further away ?
$400 Trend of ionization energy going across a period What increases (harder to remove) due to effective nuclear charge increasing (more pull - more likely to attract electrons) ?
$600 Electronegativity What energy is needed to add an electron (likeliness to gain)?
$800 effective nuclear charge and atom size What factors which affect electronegativity and how they affect it ?
$1000 Decreases.. if size is bigger, less pull from nucleus • What is the trend of electronegativity going down a family
$200 Increases due to effective nuclear charge being greater Trend of electronegativity going across a period
$400 Ionic Size Size of an ion
$600 to organize elements in meaningful way Why was periodic table developed?
$800 Mendeleev - increasing molar mass, while today’s is increasing atomic number How was Medeleevs scheme for listing elements different from that used in the modern periodic table?
$1000 elements in same group have same number of valence electrons What relationship can be seen between an elements placement within a group and its electron configuration?
$200 Noble gases had not been discovered yet due to their inactivity Why did Group 8 not appear on the Mendeleev periodic table?
$400 increasing tendency to form neg ions therefore use less energy (minus -: Exothermic Trend of electron affinity across left to right
$600 farther from nucleus therefore uses less energy to add an electron also shielding can add electrons Trend of electron affinity down top to bottom
$800 X + e− → X− Equation electron affinity
$1000 M(g) + hn ® M+ + e-. Equation for ionization energy
$200 both negative ions (right side) give off energy to gain an electron + ions use energy Electron affinity energy can be what: + or -?
$400 1) shielding 2) Effective (Strong) nuclear charge 3) add another orbit of electrons increases distance from nucleus Name 3 concepts that can affect periodicity
$600 Protons and neutrons in element 114 What exactly do these two pictures represent and where are the from?
$800 The equal the levels from the nucleus out. How do the periods on the periodic table relate to the electron orbitals and the nucleus.
$1000 1s2 2s2 2p6 3s2 3p2 and[Ne] 3s2 3p2 Long and short electron configuration for silicon.
Daily Double Dalton, Thompson, Rutherford and Bohr…Schrödinger, and Heisenberg Name the 1st five scientists in “The Atom Song
