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WorksheetsCHEM 103
Total questions: 70
Worksheet time: 54mins
He called this indivisible smallest possible piece of matter an “atom”.
Empedocles
Democritus
Aristotle
Alchemy
They believed that it could take any cheap metals and turn them into gold.
Aristotle
Democritus
Alchemy
Empedocles
He stated that all matter composed essential substances: earth, air, water and fire.
Aristotle
Democritus
Empedocles
Alchemy
He added the idea of “qualities”, the heat, cold, dryness, moisture as basic element combined.
Aristotle
Democritus
Empedocles
Alchemy
He discovered the “nucleus” of the atom with the Gold foil experiment.
Ernest Rutherford
Neil's Bohr
John Dalton
J.J. Thomson
He believed that the electrons were like plums embedded in a positively charged “pudding”.
Ernest Rutherford
Neil's Bohr
John Dalton
J.J. Thomson
He discovered the “Electron” particle.
Ernest Rutherford
Neil's Bohr
John Dalton
J.J. Thomson
He stated that all substance are made of atoms, and propose the law of conservation of mass.
Ernest Rutherford
Neil's Bohr
John Dalton
J.J. Thomson
He presented his atomic model the "energy level".
Ernest Rutherford
Neil's Bohr
John Dalton
J.J. Thomson
Is a subatomic particle which they all identical and share the nucleus with proton.
Neutrons
Protons
Electron
Nucleus
It is the core of the atom and 99% of the mass of the atom is located in this core.
Neutrons
Protons
Nucleus
Electros
Is a regular variations (or patterns) of properties with increasing atomic weight in periodic table of elements.
Period
Group
Family
Periodicity
Is a horizontal rows of elements
Period
Group
Family
Periodicity
Is an element that has characteristics properties of luster, thermal, electrical conductivity, and malleability.
Nonmetal
Metal
Metalloids
Semi metal
An elements which has physical properties of shiny and dull.
Nonmetals
Metals
Metalloids
Transition Metals
Why does effective nuclear charge steadily increases as we go from left to right across to a period?
The charge increases because the number of electrons increases but the number of core protons (shielding) stay the same.
The charge increases because the number of protons increases but the number of core electrons stay the same.
Why does effective nuclear charge increases slightly as we go down a family?
Because larger cores are less able to shield the outer electrons
Because smaller cores are much able to shield the outer electrons
This are a collection of subshells with the same principle quantum number.
Shells
Sub shells
Orbitals
Energy level
Is a region of space within an electron subshell were an electron subshell where an electron with specific energy is most likely to be found.
Shells
Sub shell
Orbitals
none of the above
Is a region of space within an electron shell that contains electrons that have the same energy.
Shell
Sub shell
Orbitals
Energy Level
This are the electrons that are located in the outermost electron shell of an element.
Shell
Valence electron
Electron shell
Electron pairing
Is a bond form between atoms of dissimilar elements (M and NM).
Ionic Bond
Covalent Bond
Metallic Bond
Mighty Bond
Covalent bond Is sharing of electrons and the resulting particle of this bond is called (a) .
(a) is the attractive force that holds the two atoms together in a more complex unit.
Molecule is a neutral group of (a) held together by chemical bonds.
Single bond is a type of covalent bond in which two atoms share (a) .
Is a type of covalent bond in which two atoms share two pairs of electrons.
Double bond
Single Bond
Triple bond
Metallic Bond
Is a type of covalent bond which approximately twice as strong a single bond.
Double bond
triple bond
single bond
metallic bond
A (a) molecule is a molecule that is made from two atoms.
Write the name of this compound: N2O
(a)
Write the name of the following compound: NaBr
(a)
(a) rule which stated that element should have contact to eight valence electrons in a bond or exactly fill up its valence shell.
The electrostatic attraction between the oppositely charged ions called (a) .
Atoms that have the same number of protons, but different neutrons are...
ions
isotopes
atoms
none of these
If electrons are added to an atom, what type of ion now exists?
anion
neutral
cation
none of the above
What does the period number tell you about an atom?
Number of valence electrons
Number of electrons
Type of element it is
Number of energy levels
Which of the following is NOT a property of metals?
Good conductors
Bendable
Good insulators
Shiny
Choose the molecule with the strongest bond.
CH4
H2O
HF
NH3
All are equal
The Cl–Kr–Cl bond angle in KrCl4 is closest to
90o
120o
360o
180o
109o
Which of the following atoms cannot exceed the octet rule in a molecule?
N
P
I
S
None of the above
Choose the electron dot formula that most accurately describes the bonding in CS2.
In the Lewis structure for ICl2–, how many lone pairs of electrons are around the central iodine atom?
0
2
4
3
What type of structure does the XeOF2 molecule have?
trigonal planar
tetrahedral
trigonal pyramidal
T-shape
According to VSEPR theory, which of the following species has a square planar molecular structure?
TeBr4
BrF3
XeF4
SCl2
If an atom gains one or more electrons, it becomes a (a) charged ion.
(a) bonds are very strong.
(a) bond does not conduct electricity in solid state but does in liquid and aqueous states.
Which of the following is Not belong in rules to remember when writing chemical formulas for ionic compounds
The symbol for the negative ions is always first.
The charges on the ions that are present are not shown in the formula. You need to know the charges to determine the formula; however, the charges are not explicitly shown in the formula.
The numbers in the formula (the subscripts) give the combining ratio for the ions.
None of the above
(a) is an ionic compound in which one element is present is a metal and the other element is nonmetal
(a) is an ion that consists of a stable group of several atoms acting together as a single charged particle.
Name the given polyatomic ion: ClO4-
(a)
Name the given polyatomic ion: ClO3-
(a)
(a) where two or more ions are held next to each other by electrical attraction.
Which of the following bonds is least polar?
C--O
I--F
Br--Br
S--Cl
Of the following, which molecule has the largest bond angle?
O3
H2O
HCN
OF2
Ionic or covalent? H2O
Covalent
Ionic
In an electron dot diagram, two pairs of shared electrons represents a (a)
What attractions hold two atoms in a molecule together?
attraction between ions with opposite charges
attraction between the molecule and other molecules
attraction between the nuclei of the atoms and shared electrons
attraction between each nucleus and the electrons of the other atom
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
A
B
C
D
JJ Thomson discovered (a) subatomic particle.
(a) was the first person to propose the concept of an atom.
Who proposed the theory that atoms orbit the nucleus in specific orbits.
Bohr
Dalton
Rutherford
Thomson
This particle balances the charges from the protons to make the atom neutral.
proton
electron
nucleus
neutron
Rutherford experimented with (a)
Thomson Experimented with (a)
(a) created this model
An atom of element X has 4 shells containing electrons. When element X reacts with chlorine, a compound with formula XCl is formed. Which of the following is the element X?
Sodium
Calcium
Oxygen
Potassium
Table shows the arrangement of electrons of elements in Period 3 of the Periodic Table. Which one of the following shows the correct descending order of their atomic radii?
M,L,N,P,K
L,M,N,K,P
P,K,N,M,L
K,L,M,N,P
Sodium and rubidium are both elements in Group 1 of the Periodic Table. Which of the following statements is correct?
Rubidium reacts less quickly with water than sodium
Rubidium has a lower melting point than sodium
Rubidium has less electrons compared to sodium
Both metals form acidic oxides
Which one of the following statements best accounts for the inert properties of Group 18 or 8 elements?
All of them have 18 elements in an atom
All of them have 8 valence electrons in each atom
Their valence shell are completely filled by electrons
All of them are rare gases and very difficult to find
