1. chemistry

    compare the emission color of lithium to that of potassium .what can you conclude about these two elements and the energy levels that their electron transition?
  2. chemistry

    (a) The characteristic emission from Ca occurs at 422.7 nm and corresponds to an electron going from a 4p orbital to a 4s orbital. Calculate the energy of the electron in the 4p orbital. Calculate Zeff for the electron in the 4p orbital. (b) The same 4p to
  3. Chem.

    Three emission lines involving three energy levels in an atom occur at wavelengths x, 1.5x, and 3.0x nanometers. Which wavelength corresponds to the transition from the highest to the lowest of the three energy levels? Please help me, thank you very much
  4. Science

    Explain, with the help of an appropriate labelled sketch diagram, how a hydrogen atom, which has only one electron, has so many spectral lines. The diagram of the energy levels follows: --------------- --------------- --------------- -----------------
  5. chemistry

    which of the following is true regarding the transition elements? A. Multiple oxidation states resulting from the involvement of d electrons in bonding is a characteristic of transition elements. B. Most transition elements have lower melting and boiling
  6. Chem

    The brilliant color of fireworks is produced by shells containing lithium carbonate (Li2CO3) that are launched into the night sky and explode. The explosions produce enough energy to vaporize the Li2CO3 and produce excited state lithium atoms. These atoms
  7. Chemistry

    What is the wavelength of the transition from n=4 to n=3 for Li2+? In what region of the spectrum does this emission occur? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels
  8. college-- chemistry

    I got stuck on this problem and I cannot figure out what to do or explain this problem. Please help me with this problem. The emission lines of one-electron atoms and ions can all be fit to the equation describing the spectrum of the hydrogen atom: E=
  9. Chemistry

    What is the wavelength of the transition from n=4 to n=3 for Li2+? In what region of the spectrum does this emission occur? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels
  10. Chem

    What is the wavelength of the transition from n=4 to n=3 for Li2+? In what region of the spectrum does this emission occur? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels
  11. Chemistry

    We did a flame testing lab today with the following metal ions: Sodium, Na^+1 Barium, Ba ^2+ Calcium, Ca ^2+ Copper, Cu ^2+ Potassium, K ^+1 Strontium, Sr ^2+ Lithium, Li ^+1 The question asks to explain the effect of the nitrate ion solution on the color
  12. Hydrogen

    Why does a hydrogen atom, which has only one electron, have so many spectral lines? Any help gratefully received. There are many energy levels the one electron can transition from/to.
  13. Physics

    When table salt is put in a candle flame, it burns bright yellow because of emission from the sodium atoms. This emission is at 590 nm. (a) What is the natural resonant frequency of the sodium atom that produces this emission (i.e. what is the
  14. Physics

    When table salt is put in a candle flame, it burns bright yellow because of emission from the sodium atoms. This emission is at 590 nm. (a) What is the natural resonant frequency of the sodium atom that produces this emission (i.e. what is the
  15. CHEM Periodic Trends

    Each of the statements below attempts to explain why some periodic property varies predictably among elements in the periodic table. Determine if each statement is true or false. Within a family, elements with higher atomic numbers have higher
  16. Chemistry (Electrons in Atoms)

    True or False. 1)Electrons give off light as they drop to lower energy levels. 2)Electrons travel around the nucleus as waves. 3)A photon of low frequency light has more energy than a photon of high frequency light. 4)Orbitals with equal energy levels each
  17. Science

    I have a question from an old exam that I need help to understand, i'm not sure where to start An electron in an electronically excited hydrogen atom undergoes a transition from a 6d to a 2p orbital, resulting in the emission of a photon. The photon
  18. science

    I have a question from an old exam that I need help to understand, i'm not sure where to start An electron in an electronically excited hydrogen atom undergoes a transition from a 6d to a 2p orbital, resulting in the emission of a photon. The photon
  19. Physical Chemistry

    26.Use Russell-Saunders LS coupling to derive the ground state levels of (a) Ne (b) F (c) Sc (d) Zr (e) C. 30. a. Construct a Grotrian diagram for the He emission spectrum (shown on the right) and use it to assign as much of this spectrum as you can using
  20. Chemistry

    I have this question from an old exam for review. I tried the question but can't get the right answers. An electron in an electronically excited hydrogen atom undergoes a transition from a 6d to a 2p orbital, resulting in the emission of a photon. The
  21. Chemistry

    I have this question from an old exam for review. I tried the question but can't get the right answers. An electron in an electronically excited hydrogen atom undergoes a transition from a 6d to a 2p orbital, resulting in the emission of a photon. The
  22. chemistry

    Examine the three listed elements of Group 13. boron (B), aluminum (Al), gallium (Ga) If boron has two energy levels, then how many energy levels do the other two elements have? Aluminum has three energy levels, and gallium has four energy levels. Aluminum
  23. chemistry

    Help plzzz Besides the major types of radioactive decay, there are two others: positron emission and electron capture. • Compare and contrast positrons with electrons. • Explain how positron emission works and how it causes transmutations. • Explain
  24. Emission Spectrum of hydrogen ...CHEM

    Can someone please explain the emissiom spectrum of hydrogen? THose lines represent the energy released by the electron when going from one orbital (energy level) to a lower orbital. The difference of energy levels exactly corresponds to the energy in the
  25. Chemistry! HELP;

    An atom of potassium (K) has 19 protons: 18 electrons in its inner electron energy levels and 1 electron in its outer energy level. What is the easiest way for this atom to get a filled outer energy level? What is formed?
  26. chemistry

    An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
  27. chemistry

    An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
  28. chemistry

    An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
  29. chemistry

    What is the wavelength of the transition from n = 2 to n = 1 for Li2+? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels of the ion are -Z2RH/n2, where Z is the atomic number.
  30. Physical Chemistry

    An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
  31. Chemistry

    According to the Bohr model, what determines the color of light emitted when an electron moves from one energy level to another? The wavelength of the photon emitted depends on the difference of the two levels the electron moved from/to.
  32. Physics

    Lithium is the atom which has three protons in its nucleus and three electrons circling the nucleus.(it usuallly has 3 nuetrons as well,but they r not important in this problem.)Two of the electrons circle the nucleus at a distance 1.8* 10^-11 m (app.)The
  33. Chemistry -Flame colors (check+help)

    What are the characteristic flame color for sodium, potassium, barium, copper, strontium, and calcium? Explain why? Ans: i know the flame colours, but for the explain why, could the below be a possible answer? The characteristic flame color is due to the
  34. Please Chemistry Help

    for the transition of an electron in a hydrogen atom between the principal quantum number levels 4 and 3, calculate a) the energy released b) the wavelength of the line in the spectra.
  35. chemistry

    if 10.3 lithium sulfate react with an abundant amount of potassium phosphate, what mass of lithium phosphate can you expect to isolate? lithium sulfate to lithium phosphate : 10.03 x 3 li3PO4 x 115.79 Lipo4 / 109.94 liSo4 / 3 LiSo4 = 10.9016179159
  36. chemistry

    help needed in drawing the diagram to show how hydrogen has numerous spectral lines I also need help with this question.... ---------------- ---------------- ---------------- ---------------- ---------------- -------------------- Each line above represents
  37. Chemistry

    Which electron transition in a hydrogen atom will emit a photon with the longest wavelength? n = 2 to n = 1 n = 3 to n = 1 n = 1 to n = 2 n = 1 to n = 3 I would assume it would be a short electron transition since energy and wavelength are inversely
  38. Chemistry (Follow up post - Dr.BOB22)

    Ionization is when an electron is removed from an atom and ionization energy is the energy required to do this. "Electrons stream from the negative electrode to the positive electrode. In the process of moving from one electrode to the other they knock
  39. biology

    Picture true of false The atom shown in the diagram has 4 energy levels or shells. 2. The atom shown in the diagram above has a total of 5 electron orbitals. 3. Each energy level consists of 2 or more orbitals. 4. The second energy level consists of 4
  40. chem

    determine the wavelength of the line in the emission spectrum produced by an electron transition He+ from ni= 4 to nf= 2.
  41. physics

    I need help with this problem so please help me. 1. A certain photoelectric surface has a threshold frequency of 6.2*10^14 Hz. A. How much kinetic energy is required to produce an electron emission? B. if the surface is illuminated with light that has a
  42. Chemistry

    What elements contains a full third energy level and what element contains the first p electron?? Here is an interactive site that will show you how the 1s, 2s, 2p, etc levels fill. Post your answers here if you want someone to check them. Also, you need
  43. Chemistry

    Which of the following elements (C, B, Be, Li for both parts of the question) will have the greatest increase in ionization energy between the removal of the first and second electrons? Which has the largest atomic radius? a. beryllium,boron b. boron,
  44. Chemistry

    Can anyone tell me why a hydrogen atom has so many spectral lines even though it has only one electron? Also how would I explain this using a diagram? There are many unfilled energy levels above ground. Excited electrons can move betwixt those levels on
  45. Physics

    Please help me answer the question below and also show equations and steps of how you came to your answer. Thank you 1. The electron in a hydrogen tom is in the first excited state, when the electron acquires an additional 2.86eV of energy. What is the
  46. physics

    Please help me answer the question below and also show equations and steps of how you came to your answer. Thank you 1. The electron in a hydrogen tom is in the first excited state, when the electron acquires an additional 2.86eV of energy. What is the
  47. chemistry please help

    Calculate the lattice energy of potassium oxide from the following data: Enthalpy of sublimation of potassium: +89.24 kJ/mol Bond energy of oxygen: +498 kJ/mol First ionization energy of potassium: +419 kJ/mol 1st electron affinity of oxygen: -141 kJ/mol
  48. CHEM please!!! help

    Calculate the lattice energy of potassium oxide from the following data: Enthalpy of sublimation of potassium: +89.24 kJ/mol Bond energy of oxygen: +498 kJ/mol First ionization energy of potassium: +419 kJ/mol 1st electron affinity of oxygen: -141 kJ/mol
  49. Chemistry

    When an electron makes a transition from the n=3 to the n=2 hydrogen atom bohr orbit, the energy difference between these two orbits (3.0x10^-19 J) is given off in a photon of light. The relationship ... between the energy of a photon and its wavelength is
  50. chemistry

    1. Write the electron configuration for each atom or ion. Then explain the distribution of electrons among energy levels. Ca, Be2+, and Br- I already found the electron configurations but I don't understand the second part of the question.(Then explain the
  51. Chemistry

    I don't understand this paragraph, can anyone explain it to me? If a large amount of energy is needed to remove an electron from an atom, the arrangement of electrons in that atom is considered to be especially stable. Thus, a high first ionization energy
  52. Chemistry

    i don't understand this paragraph, can anyone explain it to me? If a large amount of energy is needed to remove an electron from an atom, the arrangement of electrons in that atom is considered to be especially stable. Thus, a high first ionization energy
  53. Physics

    Hi I was wondering if somebody could help me with this question? According to the Bohr model, what determines the color of light emitted when an electron moves from one energy level to another? The color (wavelength) is determined by the change in energy
  54. Chem

    Which of the following pairs of elements are likely to form an ionic compound? lithium and chlorine sodium and potassium phosphorus and chlorine sodium and nitrogen argon and potassium
  55. chemistry

    The energy levels the electron can occupy in the He+ ion can be calculated using the energy level equation. Calculate the frequency (Hz) of the photon emitted when the electron goes from a n= 4.00 energy level to a n= 3 energy level. Express answer in
  56. Electron transition

    The electron in a hydrogen atom in level n= 8 undergoes a transition to a lower leve by emitting a photon of wavelength 956 mom. What is the final level of the electron? A) 4 B) 8 C) 9 D) 1 E) 3
  57. Physics

    A single electron orbits a lithium nucleus that contains three protons (+3e). The radius of the orbit is 1.76*10^-11m. Determine the kinetic energy of the electron.
  58. chemistry correction

    1. Which two elements react vigorously with each other? A: Chlorine and lithium B:Chlorine and potassium C:iodine and lithium D:iodine and potassium my answer is B 2. which statement about electronegativty is correct. A: Electronegativity decrease across a
  59. chemistry

    For the elements in row 2 of the PT discover the relationship between ionization and the family number of the element Element. Family. Ionization Ener Lithium. 1 13.6 beryllium. 2. 9.3 boron. 13. 8.3 carbon. 1 4. 11.27 nitrogen. 15 14.53 oxygen. 16. 13.62
  60. Chem

    Hello What is the wavelength (in nm) of the line in the spectrum of the hydrogen atom that arises from the transition of the electron from the orbital with n =5 to the orbital with n = 2? Note, the line corresponds to the energy of the photon that is
  61. chem

    What is the wavelength (in nm) of the line in the spectrum of the hydrogen atom that arises from the transition of the electron from the orbital with n =5 to the orbital with n = 2? Note, the line corresponds to the energy of the photon that is emitted in
  62. Chemistry

    The energy levels of one-electron ions are given by the equation: En=(-2.18*10^(-18)J)(Z^2/n^2) The series in the He spectrum that corresponds to the set of transitions where the electron falls from a higher level to the nf = 4 state is called the
  63. Chemistry

    Which sublevel begins to fill with transition elements? I don't think my guess is worthy of being posted Transition elements are in the d level.
  64. Physical Science

    If potential energy of an electron in ground state is -13.6 eV. The energy of next higher state is: a) -27.2 eV b) -6.8 eV c) -3.4 eV d) none of these please help me. Is it B? If I understand you question, yes, B is the correct answer. The energy of the
  65. CHEM AP please help!!

    Why does the octet rule not hold for many compounds containing elements in the third row of the periodic table and beyond? (Select all that apply.) 1. Atoms of elements in the third period are less subject to destabilization from additional
  66. Physics- Multiple Choice

    I need help on these 3 questions. 1. The probability that an electron will return to a lower energy level by emitting a photon is called: a. spontaneous emission b. line emission c. the Bohr radius d. the ground state I'm thinking that this one is D. 2.
  67. chemistry

    A particle wavelength (λp) of a proton is 10-12m. What is the velocity of this proton [m/s]? To achieved the velocity that you just computed, what must have been the potential difference (V) through which the proton was accelerated? An electron of
  68. chemistry

    Rank these elements according to electron affinity. Br, S, Ne most energy released by gaining an electron: most energy absorbed by gaining an electron:
  69. chemistry

    If 20 mole of potassium react with an excess of lithium sulfate , how many moles of potassium sulfate can you expect to form. porassium phosphate to potassium sulfate: 20 x 2 kaso4 x 174.259 / 212.267 /2 = 16.4188498448 lithium sulfate to potassium
  70. Chemistry

    Hi, I am having trouble determining the correct answer for this question. Which one of the following decay modes has not been observed? A)neutron emission B)Positron emission C)Alpha emission D) electron capture I don't know what does it mean be
  71. chemistry

    The energy levels the electron can occupy in the H atom can be calculated using the energy level equation. Calculate the wavelength (nm) of the photon absorbed when the electron goes from a n= 1 energy level to a n= 3 energy level. Express answer in
  72. Quantum Physics

    Each element has a different set of energy levels. Use this fact to "explain" whay the colour of the light emitted by an element in the gaseous state is characteristic of the element. When an electron falls from one of the higher energy levels to a lower
  73. chemistry

    In the emission spectrum of hydrogen, some lines are in the infra red range. h l Suggest an electron transition (specify n and n) that is in this range and calculate its corresponding wavelength and delta E.
  74. physics

    The drawing shows three energy levels of a laser that are involved in the lasing action. These levels are analogous to the levels in the Ne atoms of a He-Ne laser. The E2 level is a metastable level, and the E0 level is the ground state. The difference
  75. chemistry 1

    How do you write balanced equations A. Neutron emission by 88Br B. Electron absorption by 116Sb C. Positron emission by 184Hg D. Alpha emission by 229Th E. Neutron capture by 200Hg
  76. Chemistry

    What is the empirical distinction between emission and absorption spectra? In general terms, how did Niels Bohr explain each of these spectra? In general terms, emission spectra are obtained when the electron is at a high energy level and it falls to a
  77. physics

    If a more complicated atom has two energy levels for its electrons at (-15) eV and (-30.1) eV, what is the wavelength of the photon (in nm) that is emitted when an electron transitions between these two levels?
  78. Biology

    When the electron moves back to lower energy levels in an electron transport chain, energy is a) stored or b) released c)converted to matter d)used to make O2 I'm not sure how to answer this cause isn't it stored as potential energy of H20 and just before
  79. Chemistry

    Did I answer these correctly? 1. What is the total number of principal energy levels or shells in an atom with an atomic number of 30? a. 3 b. 4 c. 5 d. 6 I choose b. 2. The electron configuration of an atom in the ground state is 2-4. The total number of
  80. chemistry ........................chemistry

    Sodium Na+ Intense yellow Barium Ba++ Green Calcium Ca++ Brick red Copper Cu+ or Cu++ Blue-green Strontium Sr++ ? Lithium Li+ ? Sodium and potassium mixture Na+&K :yellow light Observations using the cobalt glass filter Sodium & potassium mixture
  81. physics

    Which of the following is true for the transition of electrons from a higher energy to a lower energy state? Choose one answer. a. The greater the energy difference between the levels, the more is the wavelength of the photons emitted. b. The greater the
  82. physics

    Which of the following is true for the transition of electrons from a higher energy to a lower energy state? Choose one answer. a. The greater the energy difference between the levels, the more is the wavelength of the photons emitted. b. The greater the
  83. chemistry ------ flame test-------------

    Did the nitrate ion effect the color emission of the solution ? how did you decide ? my answer: No , because The nitrate ion is the oxidizing agent in the compound without it you could not burn the chemicals and you could not produce a spectrum so there
  84. Chemistry

    An electron jumps from energy level 1 to energy level 2 by absorbing a photon of energy 8 eV. What is the most likely energy of the photon that will be emitted by the electron when it moves back down to energy level 1? 2 ev 4 ev 8 ev 12 ev What is the best
  85. Chemistry

    Calculate the energy difference (E) for the transition from n = 1 to n = 6 energy levels of hydrogen per 1 mol of H atoms. (Report your answer to at least 3 significant figures.)
  86. science

    How does a hydrogen atom have so many spectral lines when it only has one electron? That one electron can occupy many, many different energy levels.
  87. Chemistry 151

    Of the following transitions in the Bohr hydrogen atom, the ____ transition results in the emission of the highest-energy photon. a.n=1, n=6 b.n=6, n=1 c.n=6,n=3 d.n=3,n=6 e.n=1,n=4
  88. Chemistry

    The elements lithium and oxygen react explosively to from lithium oxide (Li2O). How much lithium oxide will form if 3.03 mol of lithium react? Answer in units of mol
  89. Physics

    The probability that an electron will return to a lower energy level by emitting a photon is called a. spontaneous emission b. line emission c. the Bohr radius d. the ground state I thought it was A and I looked it up online and it had A but I put it on
  90. Chemistry

    A line in the Lyman series of the hydrogen atom emission results from the transition of an electron from the n=3 level to the ground state level. a) What n level (#) is the ground state level for the hydrogen atom? b) What is the energy of this photon in
  91. Chemistry

    In regards to atomic emission spectroscopy: Explain why the intensity of the color gets brighter when the metal salt concentration is higher. Salt is any ionic compound that has positive ions(called cations) and their associated negative ions (called
  92. Chemistry

    Emission Analysis of Aqueous Solutions of Groups IA and IIA Metal Salts A student records two potassium emission spectra: 1) one using 0.10 M KNO3 solution; 2) one using 0.10 M K2SO4 solution. Will significant differences be observed in the two emission
  93. Physics

    When an electron makes a transition from its first quantum level to ground level, the energy difference is carried by the emitted photon. In comparison, how much energy is needed to return an electron at ground level to the first quantumlevel?
  94. Chemistry

    If the minimum (threshold) energy for the emission of an electron from the surface of a particular metal is 3.90 X 10-19 J, what is the kinetic energy of an electron emitted from the surface of the metal when it is irradiated by electromagnetic radiation
  95. College Chemistry

    In energy terms, ionization of an electron in an atom corresponds to the transition from whatever quantum state the electron is in to an energy of 0 KJ/mole. Calculate the energy in joules needed to remove one electron in the n=1 state from a hydrogen
  96. sicence

    The following elements as alkali, alkaline-earth or transition metals based on their positions in the periodic table: A:) iron , Fe. C:) strontium, Sr B:)potassium, k d:) platinum, Pt
  97. Chemistry

    A line in the Lyman series of the hydrogen atom emission results from the transition of an electron from the n=3 level to the ground state level. a) What n level (#) is the ground state level for the hydrogen atom? b) What is the energy of this photon in
  98. chemistry

    When a photon of light hits the surface of a metal, a photoelectron may be emitted. Some of the photon's energy is required to free the electron from the surface. The remaining energy becomes the kinetic energy of the photoelectron. The minimum energy for
  99. Physics Help Requested!

    QUESTION What is the change in energy of the hydrogen atom as the electron makes the transition from the n=3 energy level to the n=1 energy level? ANSWER xxx eV
  100. Statistics

    I need help on this one too. Any one willing to get me started? THANKS! Potassium is a mineral that helps the kidneys function normally. It also plays a key role in cardiac, skeletal, and smooth muscle contraction, making it an important nutrient for