Environmental Science Quiz Chapter 5

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to Lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What phenomenon occurs when diffracted waves interact after passing through multiple obstacles?

  • Reflection
  • Refraction
  • Interference or diffraction patterns (correct)
  • Polarization

According to the principles of the photoelectric effect, what is needed for a metal to emit electrons?

  • Any light source regardless of frequency or intensity
  • Low intensity light with a high wavelength
  • High intensity light regardless of frequency
  • A minimum frequency of light, regardless of intensity (correct)

If the energy of a photon is given by $E = hv$, how would you describe the relationship between energy and frequency?

  • Inversely proportional
  • Exponential
  • Directly proportional (correct)
  • Square root

What does the term 'binding energy' refer to in the context of the photoelectric effect?

<p>The minimum energy required to emit an electron from the metal’s surface (C)</p> Signup and view all the answers

If a metal surface ejects electrons when struck by yellow light, what is the likely outcome if it is struck by ultraviolet light?

<p>Electrons will be ejected with more kinetic energy. (C)</p> Signup and view all the answers

How many shared pairs of electrons are present in a triple bond?

<p>3 (D)</p> Signup and view all the answers

According to the general structure rules for uncharged compounds, how many bonds and unbonded pairs of electrons does an oxygen atom typically have?

<p>2 bonds and 2 unbonded pairs (B)</p> Signup and view all the answers

Which of the following elements is most likely to form two bonds and have no lone pairs in its compounds?

<p>Beryllium (Be) (A)</p> Signup and view all the answers

Which of these is NOT a typical characteristic of a halogen in a general structure?

<p>2 bonds (D)</p> Signup and view all the answers

What happens to a metal atom's outer shell when it participates in ionic bonding?

<p>It loses electrons, resulting in an empty outer shell (D)</p> Signup and view all the answers

Which of the following best describes heat capacity?

<p>The measure of a system's ability to absorb thermal energy with a change in temperature. (D)</p> Signup and view all the answers

If two substances receive the same amount of thermal energy, which substance will exhibit the smaller temperature change?

<p>The substance with higher specific heat capacity. (C)</p> Signup and view all the answers

A 200g sample of metal requires 1000 J of heat to increase its temperature by 10°C. What is the specific heat capacity ($c_s$) of the metal?

<p>0.5 J/g°C (A)</p> Signup and view all the answers

What does the molar heat of vaporization ($\Delta H_{vap}$) represent?

<p>The energy required to convert one mole of a liquid to a gas at its boiling point. (D)</p> Signup and view all the answers

A system absorbs 500 J of heat, resulting in a temperature change from 25°C to 30°C. What is the heat capacity of this system?

<p>100 J/°C (A)</p> Signup and view all the answers

Which statement is correct regarding the enthalpy change during a phase transition?

<p>The heat of vaporization is higher than the heat of fusion for a substance. (A)</p> Signup and view all the answers

If 2 moles of a substance requires 20 kJ to convert from a solid to liquid state at its melting point, what is the molar heat of fusion ($\Delta H_{fus}$)?

<p>10 kJ/mol (D)</p> Signup and view all the answers

Which scenario indicates an increase in the total thermal energy of a system?

<p>A system absorbs heat. (B)</p> Signup and view all the answers

What is the primary factor that determines the strength of temporary dipole-induced dipole forces?

<p>The ability of electrons to move around the molecule and affect neighboring molecules. (A)</p> Signup and view all the answers

Which molecular characteristic primarily enhances the strength of dispersion forces in alkanes?

<p>A greater surface-surface contact area between molecules. (A)</p> Signup and view all the answers

Compared to dispersion forces, the interactions between highly polar molecules:

<p>Are stronger due to permanent dipoles and greater attractive forces. (D)</p> Signup and view all the answers

What does the term 'miscibility' refer to regarding liquids?

<p>The capacity of a liquid to mix with another liquid without phase separation. (D)</p> Signup and view all the answers

Which condition primarily results in the formation of hydrogen bonds?

<p>Hydrogen bonded to small, electronegative atoms such as N, O, or F. (D)</p> Signup and view all the answers

What explains the unusually high boiling points of $H_2O$, $HF$, and $NH_3$?

<p>Strong hydrogen bonding. (A)</p> Signup and view all the answers

In comparison to dipole-dipole interactions, what is the relative strength of hydrogen bonds?

<p>Hydrogen bonds are significantly stronger. (B)</p> Signup and view all the answers

What is the role of ion-dipole forces in dissolving ionic substances in water?

<p>They facilitate the interactions between ions of the solute and dipoles of water molecules. (B)</p> Signup and view all the answers

Which type of intermolecular force is generally the weakest?

<p>Dispersion forces. (A)</p> Signup and view all the answers

According to 'like dissolves like' principle, which of these is most likely to occur?

<p>Ion or polar solutes dissolve in polar solvents. (A)</p> Signup and view all the answers

A substance is observed to be slightly repelled by an external magnetic field. Which term best describes this property?

<p>Diamagnetic (C)</p> Signup and view all the answers

Which of the following best describes the van der Waals radius of an atom?

<p>The radius of an atom when it is not bonded to another atom. (B)</p> Signup and view all the answers

What is the primary reason for the decrease in atomic radius observed when moving across a row (from left to right) on the periodic table?

<p>An increase in effective nuclear charge pulling electrons more strongly towards the nucleus. (D)</p> Signup and view all the answers

Why is there a relatively small change in the size of transition metals across a period compared to elements in the main group?

<p>The added electrons go to an inner (n-1) energy level which shields outer electrons, thereby not affecting the size much. (B)</p> Signup and view all the answers

Which scenario describes a paramagnetic species?

<p>An atom or ion with unpaired electrons, exhibiting an attraction to a magnetic field. (A)</p> Signup and view all the answers

What general trend in atomic radius is observed when moving down a column (group) in the periodic table?

<p>The atomic radiuses increases due to added electron shells. (D)</p> Signup and view all the answers

Compared to its neutral atom, what effect does forming a stable cation typically have on the atom's radius?

<p>The radius typically becomes smaller due to decreased electron-electron repulsion and a higher effective nuclear charge. (C)</p> Signup and view all the answers

If a neutral zinc atom (Zn) loses two electrons to form Zn$^{2+}$, which term best describes the magnetic properties of the resulting ion?

<p>Diamagnetic, because all the remaining electrons are paired. (D)</p> Signup and view all the answers

What happens to the size of cations compared to their corresponding atoms?

<p>They become smaller due to losing electrons. (A)</p> Signup and view all the answers

Which statement best describes ionization energy (IE)?

<p>IE can have multiple values for different electrons being removed. (D)</p> Signup and view all the answers

What trend occurs with first ionization energy down a group?

<p>It decreases due to electrons being farther from the nucleus. (C)</p> Signup and view all the answers

Which group has a notable exception in first ionization energy due to electron configuration?

<p>Group 3 (A), Group 6 (B)</p> Signup and view all the answers

What is electron affinity (EA)?

<p>The energy change associated with gaining an electron in a gaseous state. (B)</p> Signup and view all the answers

Which factor increases the ionization energy of an electron?

<p>Higher effective nuclear charge on the electron. (A)</p> Signup and view all the answers

Which statement is true about successive ionization energies?

<p>Particularly large increases occur when core electrons are removed. (C)</p> Signup and view all the answers

What describes why Group 6 has an easier ionization energy compared to expected?

<p>It has shared electrons in p orbitals that lead to stability. (A)</p> Signup and view all the answers

Flashcards

Heat Capacity

The ability of a system to absorb thermal energy with changing temperature.

Specific Heat Capacity (cs)

Heat required to raise 1 g of a substance by 1°C.

Molar Heat Capacity (cp)

Heat required to raise 1 mole of a substance by 1°C.

Heat Transfer Equation

q = mcΔT or q = ncpΔT for heat transfer calculations.

Signup and view all the flashcards

Molar Heat Fusion (ΔHfus)

Energy to convert 1 mole of solid at melting point to liquid.

Signup and view all the flashcards

Molar Heat of Vaporization (ΔHvap)

Energy to convert 1 mole of liquid at boiling point to vapor.

Signup and view all the flashcards

Work Calculation

1 L atm is equivalent to 101.32 J.

Signup and view all the flashcards

Thermal Energy and Kinetic Energy

Total thermal energy in a system is its kinetic energy; drops in kinetic energy lower thermal energy and temperature.

Signup and view all the flashcards

Diffraction Pattern

Pattern created when light waves interact after passing obstacles.

Signup and view all the flashcards

Photoelectric Effect

Light causes metals to emit electrons when struck, requiring minimum frequency.

Signup and view all the flashcards

Planck's Constant

A fundamental constant that relates energy of photons to their frequency, 6.626x10^-34 J s.

Signup and view all the flashcards

Energy of a Photon

Directly proportional to its frequency, can be expressed as E = hv or E = hc/λ.

Signup and view all the flashcards

Wave-Particle Duality

Light exhibits both wave-like and particle-like properties depending on the situation.

Signup and view all the flashcards

Cations

Positively charged ions that lose electrons and become smaller than their atoms.

Signup and view all the flashcards

Anions

Negatively charged ions that gain electrons and become larger than their atoms.

Signup and view all the flashcards

Ionization Energy (IE)

The energy needed to remove an electron from a gaseous atom or ion.

Signup and view all the flashcards

First Ionization Energy Trend

Increases across a period and decreases down a group due to nuclear charge and distance.

Signup and view all the flashcards

Exceptions in Ionization Energies

Certain groups show irregular IE due to electron configurations, notably Groups 3 and 6.

Signup and view all the flashcards

Second Ionization Energy

The energy required to remove a second electron, larger than the first, especially when removing core electrons.

Signup and view all the flashcards

Electron Affinity (EA)

The energy change when an atom gains an electron in a gaseous state.

Signup and view all the flashcards

Effective Nuclear Charge

The net positive charge experienced by electrons in an atom, influencing ionization energy.

Signup and view all the flashcards

Types of Chemical Bonds

Single bonds share 1 pair of electrons, double bonds share 2 pairs, and triple bonds share 3 pairs.

Signup and view all the flashcards

Determining Valence Electrons

Calculate remaining electrons using total valence - (2 x bonds).

Signup and view all the flashcards

Octet Rule Exceptions

Atoms like Be and B typically have fewer than 8 valence electrons, violating the octet rule.

Signup and view all the flashcards

Expanded Octet

Elements can have more than eight valence electrons using empty d orbitals, as in some compounds.

Signup and view all the flashcards

Ionic Bonding

Metals lose electrons to achieve noble gas configuration, leading to ionic bonds.

Signup and view all the flashcards

Paramagnetic

Materials that are attracted by an external magnetic field due to unpaired electrons.

Signup and view all the flashcards

Diamagnetic

Materials that are slightly repelled by a magnetic field, have no unpaired electrons.

Signup and view all the flashcards

Zinc Ion (Zn2+)

A diamagnetic ion formed by the loss of 2 s electrons, not paramagnetic.

Signup and view all the flashcards

Atomic Size Measurement

Measured using nonbonding (van der Waals) and bonding (covalent) radii.

Signup and view all the flashcards

Nonbonding Atomic Radius

The radius of an atom when not bonded to another atom (van der Waals radius).

Signup and view all the flashcards

Bonding Atomic Radius

Half the distance between two bonded atoms (covalent radius).

Signup and view all the flashcards

Trends in Atomic Radius

Atomic radius decreases across a row and increases down a column in the periodic table.

Signup and view all the flashcards

Induced Dipole

A temporary dipole created when molecules are close, leading to momentary attraction.

Signup and view all the flashcards

Strength of Forces

Depends on molecule size, shape, and polarizability affecting electron mobility.

Signup and view all the flashcards

Polar Molecules

Molecules with permanent dipoles due to uneven electron distribution.

Signup and view all the flashcards

Dipole Moment

A measure of the polarity in molecules based on charge separation.

Signup and view all the flashcards

Miscibility

The ability of liquids to mix without separating into layers.

Signup and view all the flashcards

Hydrogen Bonding

A stronger intermolecular force occurring when H is bonded to N, O, or F.

Signup and view all the flashcards

Boiling Points

The temperature at which a liquid turns to vapor, affected by intermolecular forces.

Signup and view all the flashcards

Ion-Dipole Interaction

Interaction between ions and polar molecules, crucial for solubility.

Signup and view all the flashcards

Solubility

The ability of a solute to dissolve in a solvent, reliant on intermolecular interactions.

Signup and view all the flashcards

Intermolecular Forces

Forces that exist between molecules, weaker than covalent bonds.

Signup and view all the flashcards

Related Documents

More Like This

Photoelectric Effect & X-Rays
30 questions

Photoelectric Effect & X-Rays

NourishingRoseQuartz avatar
NourishingRoseQuartz
Quantum Numbers & Atomic Structure
21 questions
Use Quizgecko on...
Browser
Browser