Electronegativity
Atomic Radius
Ionization Energy
So Trendy
How BohrING
A Family Grouping
I need to see some ID
Configuring the Elements
100
True or false? Electronegativity is a number that describes the relative ability of an atom, when bonded, to attract electrons. The when it trends down on the period table, it increases.
False
100
Fill in the blank. Atomic radius is defined as ________ from the outermost orbital to the nucleus
Distance
100
Which element has higher ionization energy? Carbon or aluminum
Carbon
100
The ion form of Hydrogen
H+
100
This type of model draws an atom with it's electrons separated by energy.
Bohr Model
100
Hydrogens, carbon , nitrogen are all examples of...?
non-metals
100
I determine what type of atom I am.
Protons / Atomic Number
100
A 3 dimensional region around a nucleus in which it is likely to find an electron.
What is an orbital?
200
Do electrons ever change their shell?
Yes
200
when atomic radius trends down a group why does it increase?
More orbitals; less attraction between the valence electrons and protons in nucleus.
200
Which element has higher ionization energy? Sulfer or Chlorine
Chlorine
200
How many valence electrons do elements in group 15 have and what kind of ion will they typically form?
5, anions
200
These rings represent what part(s) of an atom?
Electron Orbitals
200
Boron silicon are examples of____?
metalloids
200
The ion form of Cl
Cl-1
200
Each electron enters the lowest energy orbital available first
Aufbau Principle
300
using their location on the periodic table, determine the rank from least to greatest with the elements: Cl, Mg,Ca,N, and O
Ca,Mg,N,Cl and O
300
Define atomic radius
Is a measure of the size of its atom or the distance from the valence shell to the atom its self
300
Does the trend for ionization energy across the periodic table increase or decrease? and why?
Increase - smaller radius, electron is closer to the nucleus which makes it more difficult to pull
300
Why does it take more energy to remove the second electron from an ion than it did the first?
The effective charge of the nucleus increases, holding remaining electrons more tightly
300
What part of the periodic table describes how many energy levels this model should have?
Period / Row
300
Which trends in the periodic table increase across and decrease downwards?
electron affinity, electronegativity, ionization energy
300
I am an alkali earth metal with 3 energy levels.
Magnesium / Mg
300
How many sub-orbitals does a d-orbital have?
5
400
Predict which of the following elements has the largest En and state why? Na and Rb
sodium is higher because sodium is higher then Rb in the periodic table.
400
DAILY DOUBLE
When atomic radius trends across does it increase or decrease and why?
Decreases - has the same # of orbitals, more protons and elections therefore greater attraction and pull towards the nucleus
400
Define Ionization energy?
the energy required to remove a valence electron from an atom in its gaseous state.
400
Where are the two most reactive elements on the periodic table?
Top of the Halogens and Bottom of the Alkali metals
400
Draw a Bohr Model of a Boron Atom
400
Which trends in the periodic table increase downwards and decrease across?
Atomic radius, reactivity
400
I am the heaviest noble gas
Oganesson
400
The electron configuration of copper?
1s2 2s2 2p6 3s2 3p6 4s2 3d9
500
How does the trend go for Electronegativity and explain why
Trend down - the larger atom will pull less strongly on the electron pair since they are further to its nucleus Trend across - the smallest atom will pull more strongly on the election pair since they are closer to its nucleus
500
Using their location on the periodic table, rank the size of follwoing sets of elements in order of increasing atomic size. Mg, S, Cl,Li, Cs and K
Cl, S, Mg, K, Cs
500
In an ionization energy, when the trend goes down, what happens? and why?
the trend decrease - more orbitals, electron further from nucleus and it is easier to remove an electron
500
In general, as you go across a period in the periodic table from left to right: the atomic radius ________; the electronegativity _________; and the first ionization energy ________.
decreases, increases, increases
500
DAILY DOUBLE
Draw a Bohr model of an Argon Atom
500
Who invented the periodic table
Dmitri Mendeleev
500
I am not a metal nor non-metal and have 5 valence electrons
Antimony / Sb
Arsenic / As
500
DAILY DOUBLE
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p5
What element is this?
Iodine
9999
The shorthand notation for Uranium
[Rn]7s25f4