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UNIT 5 ATOMIC STRUCTURE , PERIODIC TABLE & RADIATION mar 2017 Flashcards | StudBud
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UNIT 5 ATOMIC STRUCTURE , PERIODIC TABLE & RADIATION mar 2017
UNIT 5 ATOMIC STRUCTURE , PERIODIC TABLE & RADIATION mar 2017
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Atomic Structure Atomic bonding Periodic Table Radiation
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1
Which of the following is the correct formula for magnesium nitrate?
Mg2(NO3)2
Mg(NO3)2
MgNO3
Mg2NO3
2
The exact number of atoms within a compound is represented by a:
Chemical Formula
Chemical Symbol
Subscript
Superscript
3
Both a fusion reaction and a fission reaction ____.
use hydrogen as a fuel
produce energy
causes chain reactions
take place at room temperature
4
A chemical reaction in which heat energy is released is ___
exothermic
endothermic
flammable
a formula
5
This equation has the same number of atoms of each element on each side of the equation
unbalanced
simple
balanced
complex
6
Numbers that precede symbols and formulas in a chemical equation are ____.
superscripts
catalysts
subscripts
coefficients
7
Thorium-234 half-life = 24 days. sample =100-g how much would remain after 48 days?
10g
100 g
50g
25g
8
A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is ____.
26
30
56
82
9
If the _____ is not great enough, the nucleus will become radioactive
Isotope
Electric Force
Strong Force
Tracer
10
T
he process by which nuclei having low masses are united to form nuclei with larger masses is
CHEMICAL REACTION
FUSION
CHAIN REACTION
FISSION
11
Substances that conduct an electric current only under certain conditions are : ____.
Noble Gases
Non Metals
metals
metalloids
12
Radioactive elements comprise a majority of the ____.
lanthanides
actinides
noble gases
halogens
13
What is the number of potassium atoms compared to oxygen atoms in a binary compound ?
One potassium atom to two oxygen atoms.
One potassium atom to three oxygen atoms.
Three potassium atoms to one oxygen atom.
Two potassium atoms to one oxygen atom.
14
Which of the following could represent a decomposition reaction?
compound + compound = compound + compound
compound = element + element
element + compound = element + compound
element + element = compound
15
The appearance of solid metals can be described as ____.
glassy
dull
powdery
shiny
16
A particle that moves around the nucleus is a(n) ____.
Quark
Proton
Neutron
Electron
17
When one element replaces another element in a compound, the reaction is a ____ reaction.
double–displacement
single–displacement
decomposition
synthesis
18
How many electrons are needed in the outer energy level for the atom to be chemically stable?
8
6
4
2
19
What is the name of the compound with the formula NaCl?
sodium dichloride
sodium chlorate
chlorine sodiate
sodium chloride
20
How does the mass of the products in a chemical reaction compare to the mass of the reactants?
The mass of the products is greater.
The masses are equal.
The mass of the reactants is greater.
There is no relationship.
21
Elements that lie along the stair-step line of the periodic table are ____.
metals
metalloids
liquids
Radioactive
22
The three types of nuclear radiation in INCREASING order of penetrating power are
X ray, gamma, beta
alpha, beta, gamma
X ray, beta, gamma
alpha, gamma, beta
23
Neutrons released in a fission reaction can strike other nuclei and cause
a chain reaction
radioactive decay
fusion reactions
an electron avalanche
24
This type of chemical reaction releases energy into its surroundings when it occurs
Exergonic
Neutralization
Hydration
Endergonic
25
The ____ tells you how many electrons an atom must gain, lose, or share to become stable.
Group number
ionic number
atomic mass
atomic number
26
Each substance on the left side of the arrow in a chemical equation is a ____.
product
reactant
catalyst
coefficient
27
Atoms of the same element with different numbers of neutrons are called
metalloids
Metals
radioactive elements
Isotopes
28
A family of elements that contains the most reactive metals is the ____.
transition elements
alkali metals
noble gases
alkaline earth metals
29
What happens when an Ionic Bond forms between a metal and non-metal?
Non Metals gain a positive charge
Metal loses electrons and Non metal gains electrons.
Non metal loses electrons and Metal gains electrons.
Metals pick up a Negative Charge
30
Which of the following is a balanced chemical equation?
AgNO3 + 2NaCl → AgCl + 3NaNO3
AgNO3 + NaCl → AgCl + NaNO3
AgNO3 + NaCl → 4AgCl + 2NaNO3
2AgNO3 + 2NaCl → 3AgCl + 2NaNO3
31
Why do the noble gases NOT form compounds readily?
They have empty outer energy levels.
They have no electrons.
They have seven electrons in the outer energy levels.
Their outer energy levels are filled with electrons.
32
Each substance to the right of the arrow in a chemical equation is a(n) ____.
inhibitor
reactant
catalyst
product
33
Horizontal rows of the periodic table are called ____
Periods
Clusters
Families
Groups
34
Elements that are gases, are brittle, and are poor conductors at room temperature are
metalloids
metals
non-metals
Isotopes
35
A chemical bond that occurs when atoms share electrons is a(n) ____ bond.
Magnetic
Ionic
Covalent
Polyatomic
36
The valence charge of an atom is shown with a ____.
negative number
positive number
subscript
superscript
37
The breaking down of a substance into two or more simpler substances is ____.
synthesis
a catalyst
displacement
decomposition
38
A group of covalently bonded atoms that acts together as one charged atom is a ____.
polyatomic ion
negative ion
molecule
crystal
39
If heat must be added to a chemical reaction for the reaction to take place, the reaction is
:
Endergonic
Balanced
Complete
Exergonic
40
What kind of chemical bond is formed when an equal exchange of electrons occurs?
magnetic
hydrate
covalent
ionic
41
In a chemical formula, the number of each atom in the compound is shown by numbers called
Subscripts
Superscripts
chemical symbols
Coefficients
42
Particles of matter that make up protons and neutrons are
quarks
atoms
electrons
isotopes
43
What type of reaction is shown in the following chemical equation: Na + Cl → NaCl
Single Replacement
Decomposition
Synthesis
Double Replacement
44
If radiation is placed near ____ cells, atoms in the cells can die or stop growing.
cancer
fat
heart
thyroid
