What is the maximum number of elnt3p a6)zx1t+dxfjxp1n q)y0 ectrons in the 4p subshell?

  What is the electron configuration of this orbital diagram?

  Which of the following subshells contains the highest energy?

  

  Which of the following is the correct electron configuration of a typical sodium ion?

  Which of the following is the correct orbital diagram for C?

  Which of the below gives the correct electron configuration of a $Cr^{3+}$ ion?

  Which equation represents the second ionization energy for Cu?

  Cobalt is an important cofactor that often inhibits enzyy not:hm-qxgpe7x :(8me activity involved in cellular respira-eq x:n xm8oyhg( t7p:tion, such as catalase.
1.Using the complete electron configuration, determine the electron configuration of Co$^{2+}$.  $s^2$  $s^2$  $p^6$  $s^2$  $p^6$  $d^7$
2.Draw the orbital diagram of the 3d electrons of Co.

  Which statements about the hydrogen emission spectrum are correct?

• 
  

  I.	The lines converge at higher energies
  II.	The lines converge at higher frequencies
  III.	The lines converge at higher wavelengths

  
  

  Which of the following statements about $^{51}_{23}V$ are correct?

I. It has 23 protons
II. It has 51 nucleons
III.It has a condensed electron configuration of [Ne]$4s^23d^3$

  Hydrogen exhibits two emission lines, D1 and D2. D1 has a wavelength a+92ux u lygv)of 656nm and D2 has a frvyal+) 9xuug2 equency $6.17\times10^{14}s^{-1}$.
1.Calculate the frequency of the D1 emission line of hydrogen.  $\times10^{14}s{-1}$
2.Calculate the wavelength of the D2 emission line of hydrogen.  $\times10^{-9}$m
3.Compare the two emission lines, and using the Data Booklet, suggest which of the emission lines is most likely to be red.

  Which statement about ionization energies is incorrect?

  1. 1.State the full electron configurations of an N atom and O atotwh6wo(0e6z,re xyhj(29 yputcfdqn* l- (;a m.N:  $s^2$  $s^2$  $p^3$ O:  $s^2$  $s^2$  $p^4$
2.Draw the orbital diagrams for an N atom and O atom.
2.Compare and explain the difference between the first ionization energy of oxygen and nitrogen.

  What will happen to the frequency of moving light particles if the wavelength is doubled, assuming the velocity is constant?

  Which of the following statements is/are true?
|. The emission spectra are produced from a release of energy of excited electrons
||. No two electrons in one atom have the same set of quantum numbers
|||. The electrons in an orbital must have an opposite spin

  Scandium is a transition metal that can form both 2+ and 3+ complexes. 7akbt9/g6 . :ibp d1m*jigkjt
1.Draw the electron in boxes notation for the 4s4s and 3d3d electrons in an Sc$^{2+}$ ion.Sc$^{2+}$(g)$\rightarrow$Sc$^{x+}$(g)+e-, x=  
2.State the equation for the third ionization energy of scandium, and indicate which electron is lost.
3.Explain why $[Sc(H_2O)_6]^{2+}$ is coloured whereas $[Sc(H_2O)_6]^{3+}$ forms a colourless aqueous solution.

  Mass spectrometry uses fast-moving electrons to ionize particles and determine the mass-to-charge ratio of an unknown compound.
1.Using the data booklet section 1 and 2, calculate the frequency of an electron with a wavelength of 1.68m.  $\times10^8s^{-1}$
2.Calculate the wavelength of an electron with a frequency of $2.00\times10^8s^{-1}$.  m
3.State the effect of increasing the wavelength on frequency.

  Deuterium is an isotope of hydrogen that contains one proton, one neutron, and one electron.

1. 1.Complete the following table.

	Protons	Neutrons	Electrons
Relative charge
Relative mass			~$\frac{1}{1836}$
Location

2.Using the following data, calculate the relative atomic mass of hydrogen correct to five decimal places, showing your work.

Isotope	Relative abundance
Hydrogen-1	99.98%
Deuterium	0.012%
Hydrogen-3	0.008%

2. 1.Describe the emission spectrum of the hydrogen atom.
2.Outline the difference between a continuous spectrum and a line spectrum.
3.Suggest how your answer to (b)(i) shows that energy levels are quantized.

  Cobalt-60 is a radioactive isotope 6d6jvf)zf:3emj+kgx 9df 2 vw of the element cobalt that is used to treat thyroid ca6jfd gfwdfmjk:9 ve26v+3 zx )ncer.
1. 1.State the full electron configuration of cobalt and chromium.
2.Explain what is special about the electron configuration of chromium.$^{60}_{27}$  
3.State the atomic symbol notation for the cobalt-60 isotope.
One atom of cobalt-60 undergoes beta decay, releasing an electron and energy with a frequency of $7.65\times10^{19}Hz$ to form nickel-60.
2. 1.Using section 1 of the data booklet, calculate the wavelength of energy released from beta decay.  $\times10^{-12}$m
2.Using section 3 (Section 5- 2025 Syllabus) of the data booklet and your answer to (b) (i), deduce the type of electromagnetic radiation emitted.
3. 1.Define orbital.
2.Sketch the shapes of an s-orbital and a p-orbital.

  Each element contains a different arrangement of electrons, and thes z o 1l)kkfvpk))2wfe.m.9 g0d1nhqlnq,/ pam e electron configurations can also penof1v2) /1h qkl kkgm. 0mp.dz,a)n 9lqwf) be represented using orbital diagrams. Determine the identity of each element described below.
1.$1s^22s^22p^63s^23p^64s^1$   
2.[Ne]$3s^23p^6$  
3.In Period 33 with valence electrons of $3^2$  
4.  

5.An ion with +1 charge, with valence electrons of:
  

  In an atom with many electrons, which set of orbitals is arranged in order of lowest electron energy to highest electron energy?

  The successive ionization energies in $kJ mol^{-1}$ for an element in the second period of the periodic table are 800, 2430, 3660, and 25000. Which element is this most likely to be?

  What is the electron configuration for the $Cu^+$ ion?

  Which of the following pairs of terms describe the shape of an s orbital and the relative energy of a d orbital?

  Which of the following ionization energies is the largest in magnitude?

  Which atoms' orbital diagram does this figure represent?

  Which of the following represents the correct ground state electron configuration of chromium?

  Molecular oxygen ($O_2$) and ozone ($O_3$) in the atmosphere undergo the following decomposition reactions.

$O_2$ $\rightarrow$O⋅+O⋅
$O_3\rightarrow$$O_2$+O⋅
The reactions occur when the reactant molecules absorb a specific wavelength of light.
Which of the following statements is true?

  Which statement about the first ionization energies for the elements in period 3 is incorrect?

  $^{63}Cu$ and $^{65}Cu$ are the two most abundant isotopes of copper.
1. 1.Define isotope.
2.Determine the correct numbers of subatomic particles to complete the following table.


3.Calculate the relative abundances of $^{63}Cu$ and $^{65}Cu$ using section 6 (Section 7- 2025 Syllabus) of the data booklet.Relative abundance of copper-63:  %Relative abundance of copper-65:  %
2.Complete the orbital diagram for the valence electrons in a copper atom and a copper (II) ion.

	Copper-63 Copper-65
Number of protons
Number of electrons
Number of neutrons

  Cu is a transition met9e5qdbu.. bxlal commonly used in wires.
1.Determine the complete electron configuration of Cu.  $s^2$  $s^2$  $p^6$  $s^2$  $p^6$  $d^{10}$  $s^1$
2.State the condensed electron configuration of $Cu^+$.  $3d^{10}$
3.Determine whether the electron configuration of Cu follows the usual rules of electron configuration.

  Which electron transition in the hydrogen atom would produce the shortest wavelength?

  John is sitting on a beach on a warm summe* 5xdd hm2r;(tc/ej pbr evening watching the reddish sky ($\lambda$=650nm) while his brother, Eric, is playing with his laser beam with a frequency of $4.60\times10^{14}s^{-1}$.
1.Calculate the frequency of the radiation from the red sky.  $\times10^{14}s^{-1}$.
2.Calculate the wavelength of the laser beam of Eric.  nm
3.Compare the wavelength of the laser beam with the wavelength of the radiation of the red sky.
4.Deduce the colour of the laser beam of Eric.

  Consider the data below on the succefl)rvk 910rq vr-drh t0uc9r6ssive ionization energies for Al.

Electrons Removed	1	2	3	4
Energy$(kJ mol^{-1})$	577	1816	2881	11600

1. 1.Explain why the successive ionization energies for an element increase.
2.Explain how the successive ionization energies for aluminium give evidence for its three valence electrons
2.Using sections 1 and 2 of the data booklet, calculate the wavelength of light required to remove an electron from an aluminium atom.  $\times10^{-7}$

  The wavelength of ligh9.h de+ xzrr9wt emitted for the n=$\infty \rightarrow$ 1 transition for an electron in a zinc atom is 296nm.
1. 1.Define first ionization energy.
2.Write an equation that represents the first ionization energy of zinc.
2.Using sections 1 and 2 of the data booklet, calculate the first ionization energy of zinc in $kJ mol^{-1}$.  $kJ mol^{-1}$

  Which of the following does NOT have two valence electrons?

  How many fully occupied p orbitals are there in selenium, Se, atom?

  Which electrons are lost in the formation of a copper (II) ion from a copper atom?

  How many unpaired electrons in the $Mn^{2+}$ ion?

  1.On the axis below, sketch the tr5p* 1::.ugtiem9f/wis aml0f uea zp,end in first ionization energies for the elements in the secoe 01gal iufme mpuf:9,*:zi/t5 a.wspnd period.


2. 1.Explain the general trend in first ionization energies.
2.Predict whether the first ionization energies for the third period elements will be  ----待选择----higherlowerthe same as  their respective elements in the second period.

  Magnesium is an element in gu+voqeow ;:b3d /k9pafbw 7;zroup 2 of the periodic table.  $s^2$  $s^2$  $p^6$  $s^2$
1.State the full electron configuration for magnesium and the block it can be found in the periodic table.
2.Explain how successive ionization energies can prove that magnesium is in group 2 and period 3 of the periodic table.
3.State the equation for the second ionization energy of magnesium.
4.State an equation for the reaction between magnesium oxide and water, and comment on the pH of the resultant solution.
5.By referring to their relative ionization energies, compare the metallic behavior of magnesium to calcium and beryllium (values from the data booklet are not required).

  Magnetic resonance imaging (MRI) is a common and powerful diagnostic tool commonly used in medicine. Imagers operate at a frequency of approximately $2.00\times10^2 MHz$.

Given the electromagnetic spectrum diagram below, in what region of the spectrum do MRI machines operate?

  Ionization energy data for the elements can be used to provide evid.goyv ;lksja 22r* 0zzence for energy levels and sublev.;yovzgs jr*k 22za 0lels within the atom.
1.The diagram below shows the amount of energy required to remove the first 10 electrons from a period 3 element.

1.Write an equation that represents the third ionization energy of an element. You can use A as the symbol for the unknown element.
2.The period 3 element is   and explain how the ionization data shown above supports your response.
3.Explain why the ionization data increases as subsequent electrons are removed from the atom
4.Write the electron configuration for the commonly formed ion of this period 3 element.  $s^2$  $s^2$  $p^6$
2.The diagram below shows the first ionization energies of the elements across period 3.

1.Explain how the first ionization data shown can be used to support the existence of the s and p sublevels of period 3.
2.Explain why Argon has such a high first ionization energy.

  The successive ionization energies for element X is sho+hkvwz1m*v c2;h*hqq9* glsiwn in the table below:
Successive Ionization Energies$(kJ mol{-1})$

1stIE	2ndIE	3rdIE	4thIE	5thIE	6thIE	7th IE	8th IE
1000	2252	3363	4556	7004	8496	27108	31724

1.Write the equation that represents the 2nd ionization energy of element X.
2.Predict the number of valence electrons for element X has   valence electrons and justify your response.
3.Another element, Y, is found below and in the same group as element X in the periodic table. The electronegativity value of element Y is 2.6. Predict a reasonable value for the electronegativity value of element X. Explain your reasoning.