Questions and Answers
Atoms with the same number of protons but with different electrical charges are called?
ions
In salt, what is the nature of the bond between sodium and chlorine?
ionic
What is the result of sodium giving an electron to chlorine?
a positively charged sodium ion and a negatively charged chlorine ion
An ionic bond involves _____?
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Hydrogen bonding is most often seen when?
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What type of bond is joining the two hydrogen atoms?
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This atom can form up to _____ single covalent bond(s).
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A(n) _____ bond joins these two oxygen atoms.
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The innermost electron shell of an atom can hold up to _____ electrons.
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Which of these relationships is true of an uncharged atom?
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What determines the types of chemical reactions that an atom participates in?
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What is the mass number of an ion with 109 electrons, 158 neutrons, and a +1 charge?
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What happens when two atoms form a chemical bond?
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What does the term electron orbital describe?
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What name is given to the bond between water molecules?
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Which statement is true of all atoms that are anions?
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The reactivity of an atom arises from?
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An ionic bond is formed when _____?
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Which property of water allows dogs to cool themselves by panting?
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What is the atomic number of an atom that has 6 protons, 6 neutrons, and 6 electrons?
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Which of these refers to atoms with the same atomic number but different atomic masses?
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Fluorine's atomic number is 9 and its atomic mass is 19. How many neutrons does fluorine have?
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An uncharged atom of boron has an atomic number of 5 and an atomic mass of 11. How many protons does boron have?
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Which of the following bonds can form between atoms of equal electronegativity?
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The atomic number of sulfur is 16. Predict the molecular formula of the compound formed when sulfur combines with hydrogen by covalent bonding.
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Which statement about weak bonds is correct?
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A carbon atom and a hydrogen atom form what type of bond in a molecule?
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Water is a source of ______________ for chemical reactions in cells.
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Which statement is true of water's tensile strength?
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Water has surface tension because...
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Which of the following best explains why water has a high specific heat?
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Which property of water molecules allows an animal to cool itself by sweating?
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Though you add heat, the temperature of boiling water remains constant because?
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Which statement helps to explain why ice is less dense than liquid water?
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Why doesn't oil mix with water?
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The type of bonding and the numbers of covalent bonds an atom can form with other atoms is determined by _____?
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What type of bond joins the carbon atom to each of the hydrogen atoms?
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Study Notes
Ions and Ionic Bonds
- Ions are atoms with the same number of protons but different electrical charges.
- An ionic bond is formed between sodium and chlorine, involving the transfer of an electron from sodium to chlorine.
- The result is a positively charged sodium ion and a negatively charged chlorine ion.
- Ionic bonds arise from the attraction between ions of opposite charges.
Hydrogen Bonds and Water Properties
- Hydrogen bonding occurs when hydrogen is covalently bonded to electronegative atoms, mainly seen in water.
- Water exhibits adhesion (clinging to surfaces) and cohesion (attraction between water molecules), contributing to surface tension.
- Water's high specific heat is due to hydrogen bonds, requiring more heat to increase its temperature compared to other substances like ethyl alcohol.
- Water can absorb substantial heat energy without a significant rise in temperature, making it effective for temperature regulation in organisms.
Atomic Structure and Bonding
- A covalent bond joins two hydrogen atoms, sharing electrons.
- Atoms can form a maximum of four single covalent bonds if they have four electrons in their outer shell.
- Double covalent bonds occur when two atoms share four electrons, as seen between oxygen atoms.
- The innermost electron shell can hold up to two electrons; the outermost shell determines an atom’s reactivity.
Charges and Isotopes
- An uncharged atom has equal numbers of protons and electrons.
- The existence of unpaired electrons in the valence shell dictates the chemical reactivity of an atom.
- Anions are atoms with more electrons than protons, while isotopes are atoms with the same atomic number but different mass numbers due to differing neutron counts.
Specific Element Details
- Fluorine has an atomic number of 9 and an atomic mass of 19, meaning it has 10 neutrons.
- Nitrogen has an atomic number of 7; an uncharged atom of this element has 7 protons and 7 electrons.
- In constructing molecular compounds, sulfur can bond with hydrogen, leading to the formula H2S, as sulfur has six valence electrons.
Water and its Unique Properties
- Water has a high heat of vaporization, allowing evaporation and cooling processes, essential for biological thermoregulation.
- The tensile strength of water results from hydrogen bonding, facilitating water transport in plants through cohesion and adhesion mechanisms.
- Ice is less dense than liquid water due to the structured hydrogen bonds formed at lower temperatures, causing unique behaviors like floating on water.
- Nonpolar characteristics of substances like oil prevent them from mixing with polar water, due to the attraction forces between polar molecules.
Subatomic Particles and Bonding
- Protons and neutrons each have a mass of approximately 1 amu; electrons have a negligible mass (about 5.5×10−4 amu).
- The type and number of covalent bonds an atom can form are also determined by the unpaired electrons present in its valence shell.
- Chemical reactions involve the breaking and forming of bonds, impacting the molecular structure and energy transformations in substances.
Summary of Chemical Bonds
- Nonpolar covalent bonds occur when atoms of equal electronegativity, while weak interactions can also exist.
- Water's high specific heat, surface tension, and evaporative cooling contribute significantly to its role in biological systems, affecting metabolism and homeostasis.
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Description
Explore the fundamental concepts of ions, ionic bonds, and hydrogen bonds within the context of chemistry. Understand how these interactions shape water's unique properties and its significance in biological systems. This quiz covers essential topics that are crucial for a solid foundation in chemistry.