Chemistry Test 1: Chapter 3 Flashcards

Questions and Answers

Which of the following elements is found in the same period of the periodic table as Sn? (Select all that apply)

Te (correct)

More than one response is correct

Which element is the first one in the group IVA (14) of the periodic table?

C (correct)

What is the symbol of the element that is in Period 4, and Group IIA (2) of the periodic table?

Ca (correct)

Silver, Ag, belongs to what period of the periodic table?

5 Signup and view all the answers

If the formula for hydrosulfuric acid is H2S, what would be the expected formula for the compound between hydrogen and tellurium, Te?

H2Te Signup and view all the answers

Which of the following statements applies to p subshells?

The p subshell is subdivided into three perpendicular shapes. Signup and view all the answers

Which of the following subshells has the highest energy?

4f Signup and view all the answers

Suppose an electron moved from the second shell to the third shell.

The move required an input of energy. Signup and view all the answers

The total number of f orbitals in an f subshell is:

7 Signup and view all the answers

The maximum number of electrons that can occupy a 3d subshell is:

10 Signup and view all the answers

The maximum number of electrons that can occupy a 4p subshell is:

6 Signup and view all the answers

What is the maximum number of electrons that can occupy the third shell?

18 Signup and view all the answers

How many electrons are in the outer shell of element 15?

5 Signup and view all the answers

Which of the following elements should have properties similar to those of nitrogen (element 7)?

P Signup and view all the answers

Which of the following has the same number of outer shell electrons as sulfur, S?

O Signup and view all the answers

What is the shell number for the outer shell electrons in bromine, Br?

4 Signup and view all the answers

Which of the following elements has an electronic configuration of 1s2 2s2 2p6 3s2 3p1?

Al Signup and view all the answers

The total number of unpaired electrons in silicon, Si, is:

2 Signup and view all the answers

Which of the following contains the same number of unpaired electrons as potassium (K)?

More than one response is correct Signup and view all the answers

Which of the following will not have electrons in the third shell?

Na+ Signup and view all the answers

Match the following pairs with the same number of electrons in the valence shell:

Na+ = Ne Signup and view all the answers

The electronic configuration of element 17 ends with:

3p^5 Signup and view all the answers

Which of the following elements contains a total of 10 's' electrons?

Sr Signup and view all the answers

What type of electron is the distinguishing electron in S?

p Signup and view all the answers

Which of the following distinguishing electrons represents an element with properties similar to an element with a 3p3 distinguishing electron?

4p^3 Signup and view all the answers

Which element is represented by the distinguishing electron configuration 3d^8?

Ni Signup and view all the answers

Which of the following elements is most likely to be a metalloid?

Ge Signup and view all the answers

Metalloids can express the characteristics of both metals and nonmetals. Which of the elements below is more likely to have the characteristics of a metal than a nonmetal?

Sb Signup and view all the answers

In which of the following elements is the distinguishing electron in a d orbital?

Cr Signup and view all the answers

Which of the following elements is classified as a transition element?

Element 76 Signup and view all the answers

Which of the following elements is classified as a representative metal?

Element 38 Signup and view all the answers

Which of the following elements is a nonmetal?

I Signup and view all the answers

Which of these elements is a gas at room temperature?

Nitrogen Signup and view all the answers

Which element has the distinguishing electron, 5p^4?

Te Signup and view all the answers

The radius of a K atom is _____ a Ca atom.

Larger than Signup and view all the answers

The melting point of oxygen is _____ selenium, Se.

Lower than Signup and view all the answers

Which of the following is a noble gas?

Neon Signup and view all the answers

The symbol of the element in period 2, group IIIA (13) is:

B Signup and view all the answers

Which element is used for relieving the symptoms of a cold?

Zn Signup and view all the answers

Which of the following statements conforms to the trends within the Periodic Table of the Elements?

Elements become more likely to be a solid at the bottom of a group. Signup and view all the answers

The highest-energy shell of an element that contains electrons is known as the:

valence shell Signup and view all the answers

_____ states that, electrons will not join other electrons in an orbital if an empty orbital of the same energy is available.

Hund's rule Signup and view all the answers

_____ explains why orbitals can contain a maximum of two electrons.

Pauli exclusion principle Signup and view all the answers

Choose the correct electronic configuration for arsenic, As.

[Ar] 4s^2 3d^10 4p^3 Signup and view all the answers

Which element has the largest atomic radius?

Cs Signup and view all the answers

The 'noble gases' is the family name for which group of the periodic table?

VIIIA (18) Signup and view all the answers

Which of the following groups belongs to the transition elements?

IIB (3) Signup and view all the answers

Which of the following is a reasonable explanation as to why atomic radii become smaller as one moves to the right for the representative elements in a period?

The charge of the nucleus increases, pulling the electron cloud closer. Signup and view all the answers

Study Notes

Periodic Table and Element Groups

Element Te is in the same period as Sn in the periodic table.
Carbon (C) is the first element in group IVA (14) of the periodic table.
Calcium (Ca) is the element in Period 4, Group IIA (2).
Silver (Ag) belongs to period 5.
The expected formula for the compound of hydrogen and tellurium (Te) is H2Te.

Electron Configuration and Subshells

The p subshell is divided into three perpendicular shapes.
The 4f subshell has the highest energy compared to 4s, 4p, and 4d.
Movement of an electron from the second shell to the third requires energy input.
An f subshell contains a total of 7 orbitals.
A 3d subshell can hold a maximum of 10 electrons.

Valence Electrons and Shell Structure

The 4p subshell can accommodate a maximum of 6 electrons.
The third shell can hold a maximum of 18 electrons.
Element 15 has 5 electrons in its outer shell.
Phosphorus (P) shares similar properties with nitrogen (N).
Oxygen (O) has the same number of outer shell electrons as sulfur (S).

Distinguishing Electrons and Unpaired Electrons

Bromine (Br) has outer shell electrons in shell number 4.
Aluminum (Al) has an electron configuration of 1s² 2s² 2p⁶ 3s² 3p¹.
Silicon (Si) has 2 unpaired electrons.
Potassium (K) and more than one element may have the same number of unpaired electrons.
Sodium ion (Na+) has no electrons in the third shell.

Relative Positions of Elements

Sodium ion (Na+) and Neon (Ne) have the same number of valence electrons.
The electronic configuration of element 17 ends with 3p⁵.
Strontium (Sr) contains a total of 10 "s" electrons.
The distinguishing electron in sulfur (S) is in the p orbital.
Elements with a 4p³ configuration have properties similar to those with a 3p³ configuration.

Classification of Elements

Nickel (Ni) corresponds to the distinguishing electron configuration 3d⁸.
Germanium (Ge) is classified as a metalloid.
Antimony (Sb) is likely to exhibit more metallic characteristics than other metalloids.
Chromium (Cr) contains a distinguishing electron in a d orbital.
Element 76 is classified as a transition element.

Properties of Elements

Element 38 is recognized as a representative metal.
Iodine (I) is identified as a nonmetal.
Nitrogen is a gas at room temperature.
Tellurium (Te) has the distinguishing electron configuration 5p⁴.
Potassium's atomic radius is larger than that of calcium (Ca).
The melting point of oxygen is lower than that of selenium (Se).

Special Groups in the Periodic Table

Neon (Ne) is classified as a noble gas.
Boron (B) is the element in Period 2, Group IIIA (13).
Zinc (Zn) is associated with relief from cold symptoms.
Elements generally become more solid as you move down a group in the periodic table.

Electron Principles and Rules

Valence shell refers to the highest-energy shell containing electrons.
Hund's rule states that electrons will occupy empty orbitals of the same energy before pairing.
The Pauli exclusion principle allows a maximum of two electrons per orbital.
Arsenic (As) has the electronic configuration [Ar] 4s² 3d¹⁰ 4p³.

Trends in Atomic Radius

Cesium (Cs) has the largest atomic radius among given options.
The noble gases belong to group VIIIA (18).
Transition elements are part of group IIIB (3).
Atomic radii decrease as one moves to the right in a period due to an increasing nuclear charge that pulls electrons closer.

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Test your knowledge with these flashcards focused on Chapter 3 of your chemistry curriculum. This quiz covers elements in the periodic table, their symbols, and positions. Perfect for review before your upcoming exam!