Quiz 3 Review (Chapter 4)

axf160030
Quiz by , created about 3 years ago

This is an unofficial Atoms First 2nd Edition Chapter 4 Quiz.

8
0
0
Tags
axf160030
Created by axf160030 about 3 years ago
Chemical Symbols
Keera
Chemistry GCSE Review - States of Matter, Particles, Atoms, Elements, Compounds and Mixtures
Morgan Overton
A2 Organic Chemistry - Reactions
yannycollins
AQA A2 English Language (B)- Child language acquisition and language change
Bethany.
A2 Geography- Water Conflicts
sophielee0909
Ionic Bondic Flashcards.
anjumn10
Electrolysis
lisawinkler10
Chemistry General Quiz - 2
lauren_johncock
Chemistry Quiz General -3
lauren_johncock
AS Chemistry - Enthalpy Changes
Sarah H-V

Question 1

Question
The color of a fire that an alkali metal gives is due to what?
Answer
  • The electron in the metal atom goes from a higher energy level to a lower energy level.
  • The metal gives off black-body radiation.
  • The metal atom ionizes.
  • The electron in the metal atom goes from a lower energy level to a higher energy level.

Question 2

Question
Which one of these sets has the elements arranged in correct order of increasing atomic radius and correctly explains the basis for this order? Hint: When electrons are being shielded (repelled) by one another, what does this do to the size of the atom?
Answer
  • Ca < Sr = Rb because size depends on the principal quantum number.
  • Sr < Rb < Ca because fewer protons mean a larger radius.
  • Ca < Rb < Sr because radius depends on the total number of subatomic particles.
  • Ca < Sr < Rb because of effective nuclear charge and number of occupied principal shells.
  • Ca < Sr < Rb because of the number of protons and the number of occupied principal shells.

Question 3

Question
Which of these operations will result in finding your Effective Nuclear Charge? Hint: Can we draw a relationship between Effective Nuclear Charge and Electron Shielding?
Answer
  • Add the number of Protons and Valence Electrons
  • Subtract the number of Valence Electrons from the number Protons
  • Subtract the number of inner/core Electrons from the number of Protons
  • Add the number of inner/core Electrons and Valence Electrons
  • Pro tip: (mac users only) Holding down Command and Control, then pushing down the space bar will let you use emojis and special characters.

Question 4

Question
An atom or ion with all electrons paired will exhibit which of these..
Answer
  • ferromagnetism
  • electromagnetism
  • diamagnetism
  • paramagnetism
  • It will reach a new energy level

Question 5

Question
How many valence electrons does a +1 cation of F (Fluorine) have? Hint: It may help to understand how Lewis Dot Structures work.
Answer
  • Over 9000
  • 9
  • 7
  • 10
  • 6

Question 6

Question
What is the very first thing you should do when you're given the name of a compound?
Answer
  • IDENTITY METALS AND NON METALS
  • PEE YOUR PANTS
  • REMOVE CAPS LOCK
  • COUNT THE NUMBER OF HALOGENS

Question 7

Question
Which one of these two elements is more likely to lose an electron than the other? Why? [Ne]3s1 [Kr]5s2, 4d10, 5p5 Think: What is the trend in Ionizing Energy, Electron affinity and Atomic Radius? Atoms with stronger ionizing energy do WHAT to weak little punks like Lithium? A bigger Atomic Radius means it's easier to do what to an atom? Where is the Atomic Radius the largest?
Answer
  • Magnesium-Mg, Because it is easier to lose one electron and achieve Noble gas stability, than to gain 6.
  • Antimony-Sb, Because it has enough Ionizing Energy, it will drop the electron and achieve Noble gas stability.
  • Sodium-Na, Because it is easier to lose one electron and achieve Noble gas stability, than to gain 6.
  • Iodine-I, In losing an electron it will reach Noble gas stability.

Question 8

Question
The electron affinity for an atom A is greater than that of atom B. What can be inferred from the given statement?
Answer
  • Atom A gains electrons more easily than atom B.
  • Atom A has fewer valence electrons than atom B.
  • Atomic radius of atom A is larger than that of atom B.
  • Atom A loses electrons more easily than atom B.

Question 9

Question
Electron affinities of fluorine (F) and chlorine are –327.8 kJ/mol and –348.5 kJ/mol respectively. Which of the following statements can be inferred from the given statement?
Answer
  • Fluorine has fewer valence electrons than chlorine.
  • The atomic radius of fluorine is larger than that of chlorine.
  • Energy is absorbed when fluorine and chlorine atoms gain an electron.
  • Energy is released when fluorine and chlorine atoms gain an electron.

Question 10

Question
Which of the following statements is true?
Answer
  • Nonmetals gain electrons readily and hence have large electron affinity.
  • Nonmetals lose electrons readily and hence have low electron affinity.
  • Metals gain electrons readily and hence have low electron affinity.
  • Metals lose electrons readily and hence have large electron affinity.

Question 11

Question
The Transition Metals are the elements in Groups 1B and 3B through 8B. Transition Metals either have incompletely filled d subshells or readily lose electrons to achieve incompletely filled d subshells. According to this definition, which group of elements are not Transition Metals? Hint: Attention to detail is key.
Answer
  • Group 9b - Zn, Cd, Hg
  • Group 2b - Cu, Ag, Au
  • Group 2b - Cu, Zn, Rg
  • Group 2b - Zn, Cd, Hg

Question 12

Question
True or False: The proccess of when an atom GAINS electrons to become an ion, is called Ionization
Answer
  • True
  • False

Question 13

Question
In drawing Lewis structures, a single line (single bond) between two elements represents?
Answer
  • an equally shared electron
  • an octet of electrons
  • an unshared pair of electrons
  • a shared pair of electrons

Question 14

Question
Which of the diatomic elements has a double bond between its atoms? HINT: one of these things is not like the other *cough* valence shell *cough*
Answer
  • oxygen
  • fluorine
  • nitrogen
  • hydrogen