K12 middle physical science chapter 7 chemical bonding2015 11-09

GradeHop Practice Test Series -
K12 Middle Physical Science Chapter 7 Chemical Bonding
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1) Identify true or false in the below sentences
A. Compounds differ in the nature of the bonds that hold their atoms
together.
B. The type of electrons in a compound determines many of its properties.
1. Both A and B are false.
2. Both A and B are true.
3. Only A is true.
4. Only B is true.
2) Fill in the blank in the below sentence
___________ can combine in ___________ different ways.
1. Elements, H
2. Elements, dioxide
3. Elements, many
4. Elements, Water peroxide
A. A chemical bond is a force of attraction between atoms or ions.
B. Examples are H for hydrogen and O for oxygen.
3. Only A is true.
4. Only B is true.
Three types of bonds are ___________, covalent, and ___________ bonds.
1. ionic, held
2. ionic, has
3. ionic, force
4. ionic, metallic
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Both carbon ___________ and carbon monoxide consist of carbon and oxygen, but
in different ratios.
1. carbon monoxide, Water peroxide
2. Water peroxide, shows
3. carbon monoxide, dioxide
4. carbon monoxide, shows
6) Identify all true sentences from the following
1. The atoms are held together by chemical bonds.
2. A chemical bond occurs when atoms share or transfer electrons.
3. The compounds are held together by chemical bonds.
4. Elements atoms join together to form molecules, crystals, or other
structures.
1. A chemical bond occurs when atoms share or transfer valence electrons.
2. A chemical bond is a force of attraction between electrons or ions.
3. There is an amazing diversity of matter in the universe, but there are
only about 100 elements.
1. Water is an example of a chemical formulas.
2. Elements can combine in many different ways.
3. The compounds are held together by chemical bonds.
2. Water is an example of a chemical compound.
4. Elements atoms join together to form molecules, crystals, or other
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structures.
11) Fill in the blanks in the below sentence
Three types of bonds are _____, _____, and _____.
1. ionic, covalent, metallic bonds
2. covalent, metallic bonds, carbon
3. ionic, metallic bonds, represented
4. ionic, metallic bonds, carbon monoxide
Both _____ and _____ peroxide consist of _____ and _____ in different ratios
of the two elements.
1. hydrogen, oxygen, metallic bonds
2. hydrogen, oxygen, represented
3. water, oxygen, hydrogen
4. water, hydrogen, oxygen
Examples are H for _____ and _____ for oxygen.
1. O, water
2. hydrogen, O
3. O, metallic bonds
4. O, represented
Water molecules always consist of two atoms of hydrogen and one atom of
oxygen Elements are _____ by chemical symbols.
1. consist of two atoms of hydrogen and one atom of oxygen Elements are,
represented
2. represented, metallic bonds
3. represented, oxygen
4. represented, O
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_____ and _____ peroxide are different compounds with different properties.
1. Water, hydrogen
2. hydrogen, represented
3. hydrogen, metallic bonds
4. hydrogen, hydrogen
A. In ionic compounds, the strong bonds between ions lock them into place in
the crystal.
B. The amount of energy needed depends on the element.
3. Only A is true.
4. Only B is true.
A. In bigger atoms, valence electrons are farther from the nucleus.
B. Ionic compounds are solids with high melting and boiling point.
3. Only A is true.
4. Only B is true.
A. By gaining an electron, the chlorine atom becomes a chloride ion.
B. The force of attraction between the negative electrons and positive
nucleus must be overcome.
3. Only A is true.
4. Only B is true.
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A. Halogens they are very reactive.
B. In bigger atoms, valence electrons are nearer to the nucleus.
3. Only A is true.
4. Only B is true.
A. Lithium iodide are excellent conductor of electricity.
B. The rigid crystals are brittle and more likely to break than bend when
struck.
3. Only A is true.
4. Only B is true.
1. Potassium chloride protect the thyriod gland from radition.
2. Opposites attract, so sodium and chloride ions attract each other.
3. Halogens they are very reactive.
4. In group 1, it takes less energy to remove an electron from lithium at
the bottom of the group than from francium at the top of the group.
1. In bigger atoms, the force of attraction between the electrons and
nucleus is weaker.
2. Opposites attract, so sodium and chloride ions attract each other.
3. Halogens they are very inactive.
4. Energy is released when an atom loose an electron and becomes a negative
ion.
1. In bigger atoms, the force of attraction between the electrons and
nucleus is weaker.
2. When ionic compounds dissolve, they release electrons and called
electrolytes.
3. Halogens release the least energy when they form ions.
4. In group 1, it takes less energy to remove an electron from francium at
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the bottom of the group than from lithium at the top of the group.
1. Ionic bonds form only between metals and nonmetals.
2. Halogens release the least energy when they form ions.
3. Less energy is needed to remove just one or a few electrons than many.
4. Calcium chloride is used to make ice.
1. The force of attraction between the negative electrons and positive
nucleus must be overcome.
2. Metals `` want '' to give up electrons, and nonmetals `` want '' to gain
electrons.
3. In group 1, it takes less energy to remove an electron from lithium at
the bottom of the group than from francium at the top of the group.
4. Bariun Iodide are given to the people who are exposed to high level of
radiation.
Ionic bonds form only between _____ and non_____.
1. nonmetals, chloride
2. nonmetals, positive nucleus
3. metals, nonmetals
4. nonmetals, snow
In bigger atoms, the force of attraction between the _____ and _____ is
weaker.
1. nucleus, high melting
2. nucleus, chloride
3. electrons, nucleus
4. nucleus, snow
An ionic bond is the force of attraction that holds together _____ and _____
ions.
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1. positive, negative
2. negative, metals
3. negative, snow
4. negative, positive nucleus
Calcium chloride is used to melt _____ and _____.
1. snow, likely
2. snow, strong
3. ice, snow
4. snow, chloride
Metals `` want '' to give up electrons, and nonmetals `` want '' to gain
electrons.
1. snow
2. boiling point
3. chloride
4. want '' to give up electrons, and nonmetals `` want '' to gain electrons
A. A polar compound is one in which there is a slight difference in charge
between opposite ends of the molecule.
B. Carbon dioxide polar.
3. Only A is true.
4. Only B is true.
A. Formaldehyde is a polar compound.
B. Many covalent compounds are gases or solid at room temperature.
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3. Only A is true.
4. Only B is true.
A. Many covalent compounds are gases or solid at room temperature.
B. In nonpolar bonds, the atoms remain neutral.
3. Only A is true.
4. Only B is true.
A. In nonpolar bonds, Neither atom attracts the shared electrons more
strongly.
B. Covalent bonds form because they give atoms a more stable arrangement of
electrons.
3. Only A is true.
4. Only B is true.
A. Shared Electrons are not free to move like the transferred electrons of
ionic compounds.
B. In a covalent bond, the shared electrons are attracted to the nuclei of
both atoms.
3. Only A is true.
4. Only B is true.
1. In nonpolar bonds, electrons are shared equally.
2. In a covalent bond, the shared electrons are attracted to the nuclei of
both atoms.
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3. In nonpolar bonds, the atoms remain neutral.
4. Many covalent compounds are gases or solid at room temperature.
1. In a covalent bond, the electrons are attracted to the nuclei of both
atoms.
2. If the covalent bonds form between atoms of different elements, a
covalent compound forms.
3. Oxygen need to share more than two pair of electrons to have a full
outer energy level.
4. In Covalent Compounds, Prefixes such as di - and tri - show the number
of each atom in the compound.
1. Covalent bonds form because they give atoms a more stable arrangement of
electrons.
2. A covalent bond is the force of attraction that holds together two atoms
that share a pair of electrons.
3. In polar bonds, electrons are not shared equally between the two atoms.
4. Covalent compounds have higher boiling points than ionic compounds.
1. Covalent compounds have different properties than ionic compounds
because of their bonds.
2. Some covalent compounds have transferred electrons.
3. Some atoms need to share more than one pair of electrons to have a full
outer energy level.
4. The oxygen atom attracts the shared electrons more strongly because its
has more positively charged electrons.
1. Some covalent compounds have transferred electrons.
2. In nonpolar bonds, electrons are shared equally.
3. In Covalent Compounds, the second element gets the suffix - ide.
4. In Covalent Compounds, the element closer to the right of the periodic
table is named first.
In Covalent Compounds, Prefixes such _____ di - and tri - show the number of
each atom in the compound.
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1. show the number of each atom in the compound, form
2. show the number of each atom in the compound, boiling
3. show the number of each atom in the compound, oxygen negative hydrogen
positive end
4. as, show the number of each atom in the compound
In Formaldehyde, one end of the molecule _____ a slightly positive charge and
other end _____ slightly negative charge.
1. form
2. has
3. as
4. oxygen negative hydrogen positive end
A bond forms between the positive hydrogen end of one water molecule and the
negative oxygen end of another water molecule is called a hydrogen bond.
1. form
2. has
3. as
4. oxygen negative hydrogen positive end
Polar covalent compounds may have _____ and _____ points than nonpolar
covalent compounds.
1. boiling, as
2. boiling, form
3. boiling, has
4. higher melting, boiling
Water is a polar compound, so its molecules are attracted to each _____ and
_____ hydrogen bonds.
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1. form, show the number of each atom in the compound
2. form, boiling
3. other, form
4. form, higher melting
A. Examples of alloys include steel, bronze, and brass.
B. Pure metals may be more useful than mixtures of metals.
3. Only A is true.
4. Only B is true.
A. Steel is an example of an alloy.
B. Alloy is formed by melting a metal and dissolving the other elements in
it.
3. Only A is true.
4. Only B is true.
A. Because of their freely moving electrons, metals are good conductors of
electricity.
B. A metallic bond is the force of attraction between a negative metal ion
and the valence electrons it shares with other ions of the metal.
3. Only A is true.
4. Only B is true.
A. The ions of the metal can move within the `` sea '' of electrons without
breaking the metallic bonds that hold them together.
B. Steel is an example of an alloy.
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3. Only A is true.
4. Only B is true.
Special bonds ___________ in ___________ that do not ___________ in other
classes of elements are called ___________ bonds.
1. form, ductile, metallic
2. form, shaped, metallic
3. form, shaped, valence electrons
4. form, metals, metallic
1. In a metallic bond, the ions are held together in the lattice by bonds
with the postive valence electrons around them.
2. In a metallic bond, the negative ions form a lattice-like structure.
3. The ions of the metal can move within the `` sea '' of electrons without
4. Special bonds form in metals that do not form in other classes of
elements are called metallic bonds.
1. In a metallic bond, the negative ions form a lattice-like structure.
with the postive valence electrons around them.
3. Metals can be shaped without breaking.
1. Metals are ductile and malleable because of the nature of their
electonic bonds.
2. In a metallic bond, valence electrons include their own and those of
other ions.
3. A metallic lattice, may resemble a rigid ionic crystal.
with the valence electrons around them.
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1. Because of their freely moving electrons and protons, metals are good
conductors of electricity.
2. The ions of the metal can move within the `` sea '' of electrons without
3. In a metallic bond, the positive ions form a lattice-like structure.
4. Metals are ductile and malleable because of the nature of their
electonic bonds.
1. Pure metals may be more useful than mixtures of metals.
2. In a metallic bond, the positive ions form a lattice-like structure.
4. A metallic bond is the force of attraction between a positive metal ion
and the valence electrons it shares with other ions of the metal.
Alloy is formed by _____ a metal and _____ the other elements in it.
1. dissolving, bronze
2. dissolving, brass
3. dissolving, those
4. melting, dissolving
In a metallic bond, valence electrons include their _____ and _____ of other
ions.
1. those, bronze
2. own, those
3. those, malleable
4. those, brass
Metals are _____ and _____ because of the nature of their metallic bonds.
1. malleable, bronze
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2. malleable, those
3. malleable, brass
4. ductile, malleable
Examples of alloys include _____, _____, and _____.
1. steel, bronze, brass
2. steel, brass, those
3. bronze, brass, melting
4. bronze, brass, dissolving
A metallic bond is the force of attraction between a positive metal ion and
the _____ it shares with other ions of the metal.
1. metal positive ion, valence electrons
2. valence electrons, bronze
3. valence electrons, malleable
4. valence electrons, brass
Answers
1. 3 2. 3 3. 2 4. 4 5. 3 6. 1,4 7. 1,3 8.
2,4 9. 2,3 10. 1,4 11. 1 12. 4 13. 2 14.
1 15. 1 16. 2 17. 2 18. 2 19. 3 20. 2 21.
2,3 22. 1,2 23. 1,4 24. 1,3 25. 1,2 26. 3 27.
3 28. 1 29. 3 30. 4 31. 3 32. 3 33. 1 34.
2 35. 2 36. 1,2 37. 2,4 38. 2,3 39. 1,3 40.
2,3 41. 4 42. 2 43. 4 44. 4 45. 3 46.
3 47. 2 48. 3 49. 2 50. 4 51. 3,4 52.
3,4 53. 2,3,4 54. 2,3 55. 2,3,4 56. 4 57. 2 58.
4 59. 1 60. 1
---End of Test---
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K12 middle physical science chapter 7 chemical bonding2015 11-09

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K12 middle physical science chapter 7 chemical bonding2015 11-09