2_Chemical_Context_of_Life_Lecture_Slides

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Chemical Context of Life Flashcards

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54 Terms

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Matter

Anything that takes up space and has mass; composed of chemical elements and compounds.

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Element

Pure substances that cannot be broken down to other substances by chemical reactions.

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Compound

Substance formed from two or more elements in fixed ratios; possess emergent properties different from those of individual elements.

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Essential elements

About 20–25% of the 92 natural elements required for life.

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Major elements

(96% of living matter): Carbon (C), Hydrogen (H), Oxygen (O), and Nitrogen (N).

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Trace elements

Elements required by an organism in only minute quantities.

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Elements in the human body (6 major)

Oxygen, Carbon, Hydrogen, Nitrogen, Calcium, Phosphorus.

(O,C,H,N,Ca,P)

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Atoms

The smallest unit of matter that compose elements consisting of protons, neutrons, and electrons.

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Neutrons

No charge

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Protons

Positive charge

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Electrons

Negative charge; surrounding the nucleus in clouds.

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Atomic number

The number of protons in an atom's nucleus.

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Mass number

The sum of protons plus neutrons in an atom's nucleus.

(proton + neutron = mass number)

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Isotope

2 atoms of the same element with different numbers of neutrons.

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Radioactive isotopes

Isotopes that decay spontaneously, giving off particles and energy. Often used in diagnostic tools in medicine.

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Cation

A positively charged ion.

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Radiometric Dating

A method used to determine the age of materials by measuring the decay of radioactive isotopes present in them.

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Energy

the capacity to cause change

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Potential energy

the energy stored in an object due to its position or arrangement.

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Electron shells

where electrons are found, each shell corresponding to a different potential energy level.

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Anion

A negatively charged ion.

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Chemical bonds

attractive forces holding atoms together

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Single bond

sharing one pair of elements

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Double bond

sharing two pairs of elements

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Nonpolar covalent bond

A type of covalent bond where electrons are shared equally between atoms, resulting in no charge separation.

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Ionic bond

The attraction between oppositely charged ions.

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Cation

a positively charged ion

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Anion

a negatively charged ion - has more electrons than protons.

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Compound

a combination of two or more different elements

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Molecule

Two or more atoms held together by covalent bonds.

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Covalent bond

The sharing of a pair of valence electrons by two atoms.

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Electronegativity

An atom's attraction for the electrons in a covalent bond.

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Polar covalent bond

A bond where one atom is more electronegative and electrons are not shared equally.

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Van der Waals interactions

weak attractions due to temporary changes in molecules

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Hydrogen bond

A weak bond formed between a hydrogen atom covalently bonded to one electronegative atom.

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Valence electrons

Electrons in the outermost shell of an atom that determine its chemical behavior.

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Chemical reaction

The making and breaking of chemical bonds.

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Reactants

The starting molecules of a chemical reaction.

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Products

The resulting molecules of a chemical reaction.

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Chemical equilibrium

When the forward and reverse reactions occur at the same rate.

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Hybrid orbitals

Orbital shapes that result from the combination of s and p orbitals.

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Molecular shape

The three-dimensional arrangement of atoms in a molecule.

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Functional groups

Specific groups of atoms within molecules that determine their chemical reactivity.

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Photosynthesis

A chemical reaction powered by sunlight that converts carbon dioxide and water into glucose and oxygen.

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Half-life

The time required for half of a sample of a radioactive isotope to decay.

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Ionic compound

Compounds formed by ionic bonds, typically found as crystals.

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Molecular mimic

A molecule that has similar structure to another and can bind to the same receptor.

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Structural formula

A representation of a molecule that shows the arrangement of atoms.

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Molecular formula

A simplified version of the structural formula that indicates the number and type of atoms.

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Bonding capacity

An atom's ability to form bonds, determined by its valence.

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Nitrogen (N) is more electronegative than hydrogen (H). Which of the following is a correct statement about the atoms in ammonia (NH3)?

a) Each hydrogen atom has a partial positive charge; the nitrogen atom has a partial negative charge.

b) Ammonia has an overall negative charge.

c) Ammonia has an overall positive charge.

d) The nitrogen atom has a partial positive charge; each hydrogen atom has a partial negative charge.

Each hydrogen atom has a partial positive charge; the nitrogen atom has a partial negative charge.

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3H2 + N2  2NH3

 

Which of the following is true for the above reaction?

a) hydrogen and nitrogen are the reactants of the reverse reaction.

b) the reaction is nonreversible.

c) ammonia is being formed and decomposed simultaneously.

d) only the forward or reverse reactions can occur at one time.

c) ammonia is being formed and decomposed simultaneously.

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Equilibrium

the rates of the reverse and forward reactions are equal.

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How many electrons are in H- and H+

2,0.