WorksheetsChemistry Quiz
Total questions: 18
Worksheet time: 9mins
An unknown element has 10 protons. Which one of the following statements is true about the element?
The element belongs in row 1 of the periodic table and is classified as a noble gas.
The element belongs in row 2 of the periodic table and is classified as a halogen.
The element belongs in row 2 of the periodic table and is classified as a noble gas.
The element belongs in row 3 of the periodic table and is classified as an alkali metal.
The list describes characteristics of four different elements: Element A is a liquid at room temperature. Element B is a solid that does not conduct electricity. Element C is a gas with an effective nuclear charge of +1. Element D is ductile and can be drawn into wires. Based on this list, which elements are metals?
Elements A and B
Elements A and D
Elements B and C
Elements C and D
Halogens are known for their high ______ because they readily ______ electrons to achieve a stable configuration.
stability; lose
reactivity; gain
inertness; gain
reactivity; lose
Arrange the following Group 1 elements in order of increasing atomic size, starting with the smallest:
Li; Na; K; Rb; Cs
Cs; Rb; K; Na; Li
Na; Li; K; Cs; Rb
Rb; Cs; Na; Li; K
Which list arranges the elements Na, Li, K, Rb, and Cs in order of decreasing ionization energy (from left (highest) to right (lowest))?
Cs; Rb; K; Na; Li
Cs; Li; Na; K; Rb
Na; Li; K; Rb; Cs
Li; Na; K; Rb; Cs
With the exception of He, how many valence electrons do noble gases have?
3
4
6
8
Beryllium is in Group 2A, Period 2 of the periodic table. Which statement describes the charge of the ion it typically forms?
It forms a cation with +2 charge.
It forms a cation with a +1 charge.
It forms an anion with a -2 charge.
It forms an anion with a -1 charge.
Consider the elements Rb, Sr, Te, Xe, and In, which are all found in Period 5 of the Periodic Table. Which sequence, from left to right, arranges them by atomic size, from largest to smallest?
Rb; Sr; Te; Xe; In
Sr; In; Rb; Xe; Te
Rb; Xe; Te; Sr; In
Rb; Sr; In; Te; Xe
Which element has 2 energy levels and is a noble gas?
He
Ne
Ar
Kr
Which element from the list has the highest electronegativity and the largest atomic radius?
F
Cs
O
Mg
Rn
Out of the list given, what element has the highest electronegativity?
F
Cl
At
Li
Fr
Which statement(s) would be expected to be true for Oganesson?
It is relatively unreactive.
It has a low ionization energy.
It has a full valence shell of electrons.
It has the largest atomic radius of the four new elements.
Both A and C.
Which of the following elements is most likely to lose electrons and form positive ions?
Nh
Ts
Mc
Og
The fact that the four new elements are Period 7 of the table means that they all:
have seven shells (energy levels) of electrons
have seven valence electrons
form ions with charges of 7+
have an effective nuclear charge of 7+
Metals are malleable which means they can be hammered into thin sheets.
True
False
The noble gases tend not to form compounds due to having a filled outer shell.
True
False
Why does the chloride ion (Cl-) have a larger radius than the chlorine atom (Cl)?
Gain of an electron increases electron-electron repulsion, leading to a larger radius.
Loss of an electron reduces electron-electron repulsion, leading to a smaller radius.
The addition of a proton increases the nuclear charge, reducing the radius.
The loss of a proton decreases the nuclear charge, increasing the radius.
When fluorine (F) gains an electron, 328 kJ of energy is released (exothermic process). If neon (Ne) gains an electron 29 kJ of energy has to be added (endothermic process). Why does this occur in both atoms?
Fluorine has a high electron affinity due to its high electronegativity and small atomic size, making it energetically favorable to gain an electron. Neon, being a noble gas with a stable electron configuration, resists gaining an electron, requiring energy input.
Fluorine and neon both have high electron affinities, but neon's electron configuration is more stable, making it energetically favorable to gain an electron.
Both fluorine and neon have low electron affinities, but fluorine's larger atomic size makes it more likely to gain an electron.
Neon has a higher electron affinity than fluorine, but its larger atomic size makes it less likely to gain an electron.
