Which represents a p orbital?

Which is correct for the line emission spectrum for hydrogen?

A. Line M has a higher energy than line N. 
B. Line N has a lower frequency than line M. 
C. Line M has a longer wavelength than line N. 
D. Lines converge at lower energy.

What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?

A. [Ar]3d⁶

B. [Ar]4s²3d⁴

C. [Ar]4s¹3d⁵

D. [Ar]4s²4p⁴

Which electron transition emits radiation of the longest wavelength?

Which represents the shape of an s atomic orbital?

Which is correct for ${}_{16}^{34}{\text{S}}^{2-}$?

What is the condensed electron configuration of the Fe²⁺ ion? 

A. [Ar]3d⁶
B. [Ar]3d⁴4s²
C. [Ar]3d⁵4s¹
D. [Ar]3d⁶4s²

What is the number of protons and the number of neutrons in ¹³¹I?

What is represented by A in ${}_{\text{Z}}^{\text{A}}{\text{X}}^{2-}$?

A. Number of electrons

B. Number of neutrons

C. Number of nucleons

D. Number of protons

Naturally occurring gallium consists of the isotopes ⁷¹Ga and ⁶⁹Ga. What is the approximate percentage abundance of ⁶⁹Ga?

M_r(Ga) = 69.72.

A.  40 %

B.  50 %

C.  60 %

D.  75 %

Which technique is used to detect the isotopes of an element?

A.  Mass spectrometry

B.  Infrared spectroscopy

C.  Titration

D.  Recrystallization

What is the relative molecular mass of bromine, according to the following mass spectrum?

NIST Mass Spectrometry Data Center Collection © 2014 copyright by the U.S. Secretary of Commerce
on behalf of the United States of America. All rights reserved.

A.  $\frac{158\times 52+160\times 100+162\times 48}{52+100+48}$

B.  $\frac{158\times 52+160\times 100+162\times 48}{158+160+162}$

C.  $\frac{79\times 11+81\times 11+158\times 52+160\times 100+162\times 48}{11+11+52+100+48}$

D.  $\frac{79\times 11+81\times 11}{11+11}$

Which is the electron configuration of a chromium atom in the ground state?

A. [Ne]3s²3p⁶4s¹3d⁴

B. [Ar]3d³

C. 1s²2s²2p⁶3s²3p⁶4s²3d⁴

D. [Ar]4s¹3d⁵

What is the maximum number of electrons that can occupy the 4th main energy level in an atom?

A.  $8$

B.  $14$

C.  $18$

D.  $32$

Which statements are correct for the emission spectrum of hydrogen?

I. The lines converge at higher frequencies.

II. Electron transitions to n = 2 are responsible for lines in the visible region.

III. Lines are produced when electrons move from lower to higher energy levels.

A.   I and II only

B.   I and III only

C.   II and III only

D.   I, II and III

In which set do all the species contain more electrons than neutrons?

A.     ¹⁴N, ¹⁶O, ¹¹C

B.     ¹⁴N, ¹⁶O, ¹¹C^4–

C.     ¹⁴N^3–, ¹⁶O^2–, ¹¹C

D.     ¹⁴N^3–, ¹⁶O^2–, ¹¹C⁴⁺

What is the relative atomic mass, $A_{\mathrm{r}}$, of an element with this mass spectrum?

A.  $24.0$

B.  $24.3$

C.  $24.9$

D.  $25.0$

Which are correct statements about the emission spectrum of hydrogen in the visible region?

I.     The red line has a lower energy than the blue line.

II.     The lines converge at longer wavelength.

III.     The frequency of the blue line is greater than the frequency of the red line.

A.     I and II only

B.     I and III only

C.     II and III only

D.     I, II and III

Which of the following is the electron configuration of a metallic element?

A.  [Ne] 3s² 3p²

B.  [Ne] 3s² 3p⁴

C.  [Ne] 3s² 3p⁶ 3d³ 4s²

D.  [Ne] 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵

Bromine consists of two stable isotopes that exist in approximately a 1 : 1 ratio. The relative atomic mass, A_r, of bromine is 79.90. Which are the stable isotopes of bromine?

A. ⁷⁹Br and ⁸¹Br

B. ⁸⁰Br and ⁸¹Br

C. ⁷⁸Br and ⁸⁰Br

D. ⁷⁹Br and ⁸⁰Br

What does ${}_{12}^{24}M{g}^{2+}$ represent?

A.     An ion with 12 protons and 24 neutrons

B.     An ion with 14 protons and 24 neutrons

C.     An ion with 12 protons and 12 neutrons

D.     An ion with 12 protons and 22 neutrons

Which statement about ⁵⁶Fe³⁺ and ⁵⁴Fe²⁺ is correct?

A. Both have the same numbers of protons and electrons.

B. Both have the same number of protons.

C. Both have the same number of neutrons.

D. Both have the same numbers of protons and neutrons.

The full electron configuration of an element is:

1s²2s²2p⁶3s²3p²

To which group and period does the element belong?

What is the relative atomic mass of an element with the following mass spectrum?

A.  23

B.  24

C.  25

D.  28

How are emission spectra formed?

A.  Photons are absorbed when promoted electrons return to a lower energy level.

B.  Photons are absorbed when electrons are promoted to a higher energy level.

C.  Photons are emitted when electrons are promoted to a higher energy level.

D.  Photons are emitted when promoted electrons return to a lower energy level.

What is represented by ^“2−” in ${}_{\mathrm{Z}}{}^{\mathrm{A}}\mathrm{X}^{2-}$?

A.  loss of electron

B.  gain of electron

C.  loss of proton

D.  gain of proton

Which experimental results support the theory that electrons exist in discrete energy levels?

A.  ¹H NMR

B.  X-ray diffraction pattern

C.  Emission spectra

D.  IR spectra

What is the composition of the nucleus of ²⁶Mg?

How many p-orbitals are occupied in a phosphorus atom?

A.  2

B.  3

C.  5

D.  6

Which electron transition in the hydrogen atom emission spectrum emits radiation with the longest wavelength?

A.     n = 2 → n = 1

B.     n = 1 → n = 2

C.     n = 4 → n = 1

D.     n = 3 → n = 2

What is the maximum number of electrons that can occupy a p-orbital?

A.  2

B.  3

C.  6

D.  8

Which transition in the hydrogen atom emits visible light?

A. n = 1 to n = 2

B. n = 2 to n = 3

C. n = 2 to n = 1

D. n = 3 to n = 2

Which shows the number of subatomic particles in ³¹P³⁻?